Chemical Equation for Silver lab Cu (s) + 2AgNO 3 (aq) 2Ag (s) + Cu(NO 3 ) 2 (aq) Ionic Equation for Silver Lab (with Spectator Ions) Cu (s) + 2Ag 1+ (aq) + 2NO 3 1- (aq) 2Ag (s) + Cu 2+ (aq) + 2NO 3 1- (aq) Net Ionic Equation for Silver Lab (without Spectator Ions) Cu (s) + 2Ag 1+ (aq) 2Ag (s) + Cu 2+ (aq) Writing Net-Ionic Equations
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Writing Net-Ionic Equations...Net Ionic Equation for Silver Lab (without Spectator Ions) Cu (s) + 2Ag1+ 2+(aq) 2Ag (s) + Cu (aq) Writing Net-Ionic Equations Net-Ionic Equation Spectator
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Chemical Equation for Silver lab
Cu (s) + 2AgNO3 (aq) 2Ag (s) + Cu(NO3)2 (aq) Ionic Equation for Silver Lab (with Spectator Ions) Cu (s) + 2Ag1+ (aq) + 2NO3
1- (aq) 2Ag (s) + Cu2+ (aq) + 2NO31- (aq)
Net Ionic Equation for Silver Lab (without Spectator Ions) Cu (s) + 2Ag1+ (aq) 2Ag (s) + Cu2+ (aq)
Writing Net-Ionic Equations
Net-Ionic Equation
Spectator Ions
Anode Cathode
Cu0 Cu2+ + 2e- Ag1+ + 1e- Ag0
Anode Cathode
Cu0 Cu2++ 2e- Ag1+ + 1e-
Ag0
Eo = -0.34 V Eo = +0.80 V
Oxidation Process Reduction Process
Reducing Agent Oxidizing Agent
Cu(s) | Mg2+ (1.0 M) || Ag1+(1.0 M) | Ag (s)
Eocell = +0.46 V
Anode Cathode
Zn0 Zn2+ + 2e- Ag1+ + 1e- Ag0
The short-hand chemistry notation used to represent the electrochemical cell redox
reaction shown in the previous illustration is written as
Zn (s) | Zn2+ (1.0 M) || Cu2+ (1.0 M) | Cu (s)
By convention, the half-cell with the anode, undergoing oxidation, is placed to the left.
The half-cell with the cathode, undergoing reduction, is placed to the right of the
double-vertical line. The standard-state ion concentrations are 1-M concentrations.
Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V
Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V
Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V
Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V
Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V
Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V
Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V
Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V
Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V
Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V
Cu2+(aq) + 2e- = Cu(s) Eooxidizing agent = +0.34 V