Electrochemistry is the study of chemical reactions that produce electrical effects.

Electrochemistry is the study of chemical reactions that produce electrical effects

General Information

bull Charge ndash property of matter

bull There are two kinds of chargendash electron rarr -160 x 10-19 C

ndash proton rarr +160 x 10-19 C

bull 10 Coulomb of charge is equivalent to 625 x 1018 electrons

General Information

bull Currentndashflow of charge

ndashmeasured in amperes (A)

bull 1 Ampndashflow of 10 C of charge per second

past a given point (Cs)

General Information

bull Circuitndasha closed pathway for charge to

travel

ndashmay be a solid or fluid path

Conductors in which only electrons can move

Solution of positive and negative ions that are free to move

Voltaic Cell

bull harnessed chemical reaction which produces an electric current

bull converts chemical potential energy into electrical potential energy

Voltaic Cell

bull Salt bridge (U-tube)ndash connects the two half cellsndash allows ions to be exchanged but prevents

mixing of the solutions

bull This reaction is spontaneousndash oxidation (RA) rarr Zn(s) harr Zn+2

(aq) + 2e-

ndash reduction (OA) rarr Cu2+(aq) + 2e- harr Cu(s)

Voltaic Cell

bull The two metal rods are called electrodes this is where the electrons enter and leave the cellndash The electrode where oxidation occurs is

called the anodendash The electrode where reduction occurs is

called the cathode

Voltaic Cell

bull Anodendash electrons leave the cell from the anodendash positive ions are produced

ndash Zn(s) rarr Zn2+(aq) + 2e-

bull Cathodendash electrons enter the cathodendash solid metal is produced

ndash Cu2+(aq) + 2e- rarr Cu(s)

Voltaic Cell

anode cathode

Voltaic Cell

bull At any time in a given half cell electrical neutrality is maintained by the movement of ions across the salt bridge

bull Negative ions (anions) drift toward the anode

bull Positive ions (cations) drift toward the cathode

The ZnCu Voltaic Cell

Problem

bull Draw a diagram of a copperaluminum voltaic cell Label the anode and cathode and show the direction of electron flow Write the equations for the reactions that occur and predict the cell voltage

Solution

bull Locate the reactions in data bookndash Cu2+

(aq) + 2e- rarr Cu(s) +034

ndash Al3+(aq) + 3e- rarr Al(s) -166

bull For a voltaic cell reverse the lower reaction ( Al is lower on table ndashoxidized)ndash Cu2+

(aq) + 2e- rarr Cu(s) +034

ndash Al(s) rarr Al3+(aq) + 3e- +166

Net ionic reactionCu2+ (aq) + 2e- lt - gt Cu (s)

Al(s) lt - gt Al3+(aq) + 3e-

Remember in all redox equations the electrons are removed

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

3 Cu2+ + 2 Al(s) lt - gt 3 Cu(s) + 2Al3+(aq)

copper aluminum

Cu2+ Al3+

Voltaic Cellbull the shorthand representation of an

electrochemical cell showing the two half-cells connected by a salt bridge or porous barrier such as

Zn(s)ZnSO4(aq)CuSO4(aq)Cu(s)

anode cathode

Phase boundary

Liquid junction

Remember

bull Redox reactions can be viewed as a competition for electrons Therefore the reaction is always between the strongest oxidizing agent and the strongest reducing agent

Problem

bull A strip of metal X is placed in XNO3 solution It makes an electrochemical cell with Al3+

(aq) half cell It is observed that Al(s) is deposited on the aluminum electrode and the cell voltage is 075 V Calculate the reduction potential of X

Solution

bull Al is reduced Al3+(aq) + 3e- rarr Al(s) -166

bull X is oxidized X(s) rarr X+(aq) + e-

bull Solve for -166 + = +075

= 241 VX is being oxidized reduction potential is ndash 241 V

( ) x 3

Al3+(aq) + 3X(s) rarr Al(s) + 3X+

(aq) 075

WS 15-2

Standard Electrode Potentials

bull A measure of the relative tendency of substances to gain electrons

bull The standard was chosen to be the hydrogen half cell

bull The hydrogen half cell was chosen to be zero This does not mean H+ will not gain electrons

Hydrogen Electrode

bull consists of a platinum electrode covered with a fine powder of platinum around which H2(g) is bubbled Its potential is defined as zero volts

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

bull Since the hydrogen half cell has a relative value of 000 V any half cell connected to it will have its standard potential read off of the voltmeter that connects the two half cells

A Voltaic Cell With Zinc and the Standard Hydrogen Electrode

[Zn2+]= [H+] = 1000 M

bull Any half cell that gives up electrons to H+ will have a negative potential since it has less potential to gain electrons than H+

bull Any half cell that takes electrons from H2(g)

has a positive potential since it has a greater potential to gain electrons than H+

bull ExamplesndashCuCu2+ rarr Eo = 034 V 034 V

greater potential than H+H2

ndashAlAl3+ rarr Eo = -166 166 V less potential than H+H2

If the reduction of mercury (I) in a voltaic cell is desired the half reaction is

Which of the following reactions could be used as the anode (oxidation)

WS 15-22

Multiple cells

bull If the cells are connected to the anode then add the potentials

bull If the cells are connected at the cathode then subtract the potentials

Electrolytic cells

bull Electrical energy is converted to chemical energy

bull Non-spontaneous reactions

bull Reaction is still between the strongest OA and RA (OA is not strong enough)

bull Require outside energy source

Electrolytic cells

bull The Eo value for an electrolytic cell is negative

bull The Eo value is the minimum voltage that must be applied to the cell to force it to react

Electrolytic cells

bull In diagramsndashcell with ammeter rarr voltaic

ndashcell with battery rarr electrolytic

anode (+)cathode (-)

ElectroplatingElectrolysis

Electroplating is the process of

1) Current = rate of flow of charge

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

current (A) charge (C)

time (s)

Q = 965 x 104 Cmol (Faradayrsquos constant)

5) To calculate number of mol of electrons

ne = q Q

ne = 18000 C 965 x 104 Cmol

ne = 01865 mol of e-

250 A of current runs for 20 hours through a silver nitrate solution Find the mass of silver produced

q = Itq = (250 A) x (7200 s)q = 18 000 C

Ag+(aq) + 1e- rarr Ag(s)

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

I rarr current (Amps)

t rarr time (s)

M rarr molar mass (gmol)

Q rarr molar charge (Cmol)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

A person wants to plate an ornament with 100 g of silver The ornament is placed in a salt of silver and a 15 A current is placed through the solution The voltage is 100 How long will the plating process take

Copper plating a key

inert anodecathode

Molten or Aqueous

Aqueous

bull NaCl rarr Na+ + Cl-

bull Species present

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

bull Calculate the net potentials and write the reactions that occur whenndash NaI(s) is electrolyzed

ndash A solution of NaI(aq) is electrolyzed

NaI(s) is electrolyzed

Na+(l) I-

Na+(l) + e- rarr Na(s) -271

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

A solution of NaI(aq) is electrolyzed

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

2H2O(l) + 2I-(aq) rarr H2(g)+ 2OH-

(aq) + I2(s) -137

Electrolysis of Brine

H2O OA

2H2O(l) + 2Cl-(aq) rarr H2(g) + 2OH-(aq) + Cl2(g)

bull The Cl- ion is a stronger reducing agent than H2O during electrolysis of brine even though the table indicates that it is not

Electrolysis of molten NaCl

Changing Concentration

bull A change in concentration around the cathode or anode will change the value of Eo for half cells

Cu(s) rarr Cu2+(aq) + 2e-

bull An increase in concentration of copper ions will cause a shift to the left making less products

bull Increase in concentration around anode causes a decrease in Eo

Cu2+(aq) + 2e- rarr Cu(s)

bull An increase in concentration of copper ions will cause a shift to the right making more products

bull Increase in concentration around cathode causes a increase in Eo

Cathode

bull Since E(Fe2+Fe) lt E(O2H2O) iron can be oxidized by oxygen

bull Cathodendash O2(g) + 4 H+

(aq) + 4 e- 2 H2O(l)

bull Anode ndash Fe(s) Fe2+

(aq) + 2 e-

bull Fe2+ initially formed ndash further oxidized to Fe3+ which forms rust

Rusting (Corrosion) of Iron

Preventing the Corrosion of Iron

bull Corrosion can be prevented by coating the iron with paint or another metal

bull Galvanized iron - Fe is coated with Znbull Zn protects the iron (Zn - anode and Fe -

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

To protect underground pipelines a sacrificial anode is added

The water pipe - turned into the cathode and an active metal is used as the sacrificial anode

Mg is used as the sacrificial anode

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Corrosion Prevention

Living Battery

bull The eel generates electric charge in a battery of biological electrochemical cells each cell providing about 015 V and an overall potential difference of ~ 700 V Note that the eels head is the cathode(+) and its tail the anode(-) The cells extend over the length of the eel

Types of Batteries

Batteriesndash device that converts chemical energy into electricity

Primary Cellsndash non-reversible electrochemical cellndash non-rechargeable cell

Secondary Cellsndash reversible electrochemical cellndash rechargeable cell

Types of Batteries

Primary Cells

dry cell amp alkaline cell 15 vcell

mercury cell 134 vcell

fuel cell 123vcell

Secondary Cells

lead-acid (automobile battery) 2 vcell

NiCad 125 vcell

Lead-Acid Battery

bull A 12 V car battery - 6 cathodeanode pairs each producing 2 V

Cathode PbO2 on a metal grid in sulfuric acid

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

A Picture of a Car Battery

An Alkaline Battery

bull Anode Zn cap

Zn(s) Zn2+(aq) + 2e-

bull Cathode MnO2 NH4Cl and carbon paste

2 NH4+

(aq) + 2 MnO2(s) + 2e- Mn2O3(s) + 2NH3(aq) + 2H2O(l)

bull Graphite rod in the center - inert cathode

bull Alkaline battery NH4Cl is replaced with KOH

bull Anode Zn powder mixed in a gel

ldquoDryrdquo Cell

The Alkaline Battery

ldquoNewrdquo Super Iron Battery

BaFeO4 + 32 Zn rarr 12 Fe2O3 + 12 ZnO + BaZnO2

Environmentally friendlier than MnO2 containing batteries

Fuel Cells

bull Direct production of electricity from fuels occurs in a fuel cell

bull H2- O2 fuel cell was the primary source of electricity on Apollo moon flights

bull Cathode reduction of oxygen

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

General Information

bull Charge ndash property of matter

bull There are two kinds of chargendash electron rarr -160 x 10-19 C

ndash proton rarr +160 x 10-19 C

bull 10 Coulomb of charge is equivalent to 625 x 1018 electrons

General Information

travel

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

General Information

travel

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

General Information

travel

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

(aq) + 2e-

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

called the cathode

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

anode cathode

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Voltaic Cell

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Problem

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Solution

(aq) + 2e- rarr Cu(s) +034

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

3 Cu2+ + 6e- lt - gt 3 Cu(s)

2 Al(s) lt - gt 2Al3+(aq) + 6e-

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

copper aluminum

Cu2+ Al3+

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

anode cathode

Phase boundary

Liquid junction

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Remember

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Problem

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Solution

( ) x 3

(aq) 075

WS 15-2

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Hydrogen Electrode

Hydrogen Half-Cell

H2(g) rarr 2 H+(aq) + 2 e-

reversible reaction

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Hydrogen Electrode

Non reactive

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

[Zn2+]= [H+] = 1000 M

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

WS 15-22

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Multiple cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Electrolytic cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

2) I = q t

3) 1 e- = 16 x 10-19 C

4) 1 mol e- = 602 x 1023 e- x 16 x 10-19 C

= 965 x 104 C

time (s)

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

ne = q Q

ne = 18000 C 965 x 104 Cmol

q = Itq = (250 A) x (7200 s)q = 18 000 C

01865mol 01865 mol

m = n x M

m = 01865 mol x 10787 gmol

m = 20 g

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Short cut

m = I t M

m = (250 A) (7200 s) (10787 gmol) (965 x 104 Cmol) (1)

m = 20 g

t rarr time (s)

V rarr voltage

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

m = I t M

100 g = (150 A) t (10787 gmol) (965 x 104 Cmol) (100)

t = 59639589 s = 166 h

WS 15-33

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

inert anodecathode

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Molten or Aqueous

Aqueous

ndash Na+(aq)

ndash Cl- (aq)

ndash H2O(l)

Molten

ndash Na+(l)

ndash Cl- (l)

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Na+(l) I-

2I-(l) rarr I2(s) + 2e- -054

2Na+(l) + 2I-

(l) rarr 2Na(s) + I2(s) -325

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

H2O(l) Na+(aq) I-

2H2O(l) + 2e- rarr H2(g)+ 2OH-(aq) -083

2I-(aq) rarr I2(s) + 2e- -

(aq) + I2(s) -137

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

H2O OA

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Cathode

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

(aq) + 4 e- 2 H2O(l)

(aq) + 2 e-

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

the cathode)

Zn2+(aq) +2e- Zn(s) E(Zn2+Zn) = -076 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Mg2+(aq) +2e- Mg(s) E(Mg2+Mg) = -237 V

Fe2+(aq) + 2e- Fe(s) E(Fe2+Fe) = -044 V

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Living Battery

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Types of Batteries

Primary Cells

fuel cell 123vcell

Secondary Cells

NiCad 125 vcell

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Lead-Acid Battery

PbO2(s) + SO42-

(aq) + 4H+(aq) + 2e- PbSO4(s) + 2H2O(l)

Anode Pb

Pb(s) + SO42-

(aq) PbSO4(s) + 2e-

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

An Alkaline Battery

bull Anode Zn cap

2 NH4+

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

2 H2O(l) + O2(g) + 4 e- 4 OH-(aq)

bull Anode

2 H2(g) + 4 OH-(aq) 4 H2O(l) + 4 e-

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

General Information

Voltaic Cell

Problem

Solution

Net ionic reaction

Remember

Hydrogen Electrode

Multiple cells

Electrolytic cells

Short cut

Molten or Aqueous

Living Battery

Types of Batteries

Lead-Acid Battery

An Alkaline Battery

ldquoDryrdquo Cell

Fuel Cells

Electrochemistry is the study of chemical reactions that produce electrical effects.

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