Q of the Day

1. Locate your Chapter # 3 Quest.

2. Calculate and record your % grade.

3. Did you meet your goal? Why or why not.

4. Study (preparation) Plan for next test?

5. Record your new goal:

- Average your first three tests (or quests) and improve by at least two!

Day 6 11-18

33,600 mL of Helium = ____ atoms at STP

Day 1 11-19

P1V1 = P2V2

DAY 2 11-201. What is Boyle’s law? _____________ 2. Why are temperatures around zero

Kelvins bad for an ideal gas?

PERIODS 1 and 2

Day 2 11-20

1. Gases consist of large #s of tiny particles that are far apart relative to their size (each particle has mass)

Kinetic-molecular Theory - Gases

2. Collisions between gas particles and between particles and container walls are elastic

3. Gas particles are in constant, rapid, random motion… they possess kinetic energy

Kinetic-molecular Theory - Gases

4. There are no forces of attraction or repulsion between gas particles

5. The average kinetic energy of gas particles depends on the temperature of the gas

The Gas LawsBoyle’s Law: – Pressure-volume relationship – the volume of a fixed mass of gas varies inversely with the pressure at constant temperature

Comparing conditions:

P1V1 = P2V2

Boyle’s Law:

Constant n and T

P and V change

The Gas LawsCharles’ Law: – Volume-temperature relationship – the volume of a fixed mass of gas varies directly with the Kelvin temperature at constant pressure

Comparing conditions:

V1/T1 = V2/T2

Temperature decrease

Charles’ Law: –

Constant n and P

T and V change

The Gas LawsGay-Lussac’s Law: – Pressure-temperature relationship – the pressure of a fixed mass of gas varies directly with the Kelvin temperature at constant volume

Comparing conditions:

P1/T1 = P2/T2

Low T - Slow moving

High T - Fast moving

Temperature Increase

Gay-Lussac’s Law: –

Constant n and V

T and P change

The pressure exerted on a 3 L sample of gas is 600 mm Hg, if the pressure is decreased to 300 mm Hg what is the new volume?

1.Highlight important info.

2.Choose a law

3. Identify conditions as beginning (1) or ending (2)

4.Solve

At 100 K a sample exerts a pressure of 2.026e5 Pa, if the pressure is decreased to 1.013e5 Pa what is the new temperature?

What law do you use? __________________

Solve:

Gay-Lussac’s: P1/T1 = P2/T2

Whose Law

P1/T1 = P2/T2

P1V1 = P2V2

V1/T1 = V2/T2

Gay-Lussac’s

Boyle’s

Charles’

Africa’s killer lakes:

http://natgeotv.com/uk/killer-fog/videos/tragedy-at-lake-nyos

http://www.youtube.com/watch?v=LcPg7HyTWnM&feature=related

http://www.youtube.com/watch?v=ppbcl-MP76s

Lab Reports and Presentations are due on Wednesday 12-4

Postlabs are due on Friday 11-22

Review section 14.2 and complete #s 17-19, 22, 24, + 25 on page 463

- DUE WEDNESDAY 11-20

DAY 2 11-28

2. Write a Boyle’s law problem (word problem) in your notebook with the answer

1. At 100 K and 1 atm a sample has a volume of 2L, if the gas expands to 6L what is the new temperature?

Not in notes

Specifically explain what happened in Part A of your lab (it will help to get your lab out).

*** This will be important for your lab report, presentation, or postlab!

Day 4-11-30

PERIOD 1

PERIOD 3

Describe Dalton’s law.

Day 3 12-7

Ideal gas law – mathematical relationship of pressure, volume, temperature, and the # of moles of a gas

PV = nRT

R = the ideal gas constant = 8.314

Page 454 table 13.2

L * kPamol * K

http://en.wikipedia.org/wiki/Gas_constant

What pressure in atms. is exerted by 0.325 mol of hydrogen gas in a 4.08 L container at 35°C?

1. Convert to Kelvins

2. Choose R

3. Solve

0.0821 atm-L/mol-K

8.314 J/mol-K

PV = nRT

1. If a balloon is in this room (about 1 atm. and 300 K) and its volume is 0.40 L, how many moles of gas does it contain?

On notes page 6

What mass of chlorine gas in grams is contained in a 10.0 L tank at 27°C and 3.50 atm of pressure?

101 gOn notes page 5

What is the volume occupied by 4.67 moles of H2 at 27.0 °C and 2.00 atm.?

On notes page 6

3.3 mols Cu(NO3)2 X = 4.4 mols H2O3 mols Cu(NO3)2

4 mols H2O

2.0 mols HNO3 X X = 48 g Cu8 mols HNO3

3 mols Cu

1 mol Cu

63.5 g Cu

4.0 g H2 X X X = 32 g CH 3OH2 g H2

1 mol H2

2 mols H2

1 mol CH3OH

1 mol CH3OH

32 g CH3OH

X 100 = 88%32 g CH3OH

28.0 g CH3OH

4 mols Na X = 2 mols Cl22 mols Na

1 mol Cl2

3.50 g Na3PO4 X X X = 8.35 g Ba(NO 3)2164 g Na3PO4

1 mol Na3PO4

2 mols Na3PO4

3 mols Ba(NO3)2

1 mol Ba(NO3)2

261 g Ba(NO3)2

6.4 g Ba(NO3)2 X X X = 4.9 g Ba 3(PO4)2261 g Ba(NO3)2

1 mol Ba(NO3)2 1 mol Ba3(PO4)2

3 mols Ba(NO3)2

602 g Ba3(PO4)2

1 mol Ba3(PO4)2

X 100 = 102%4.9 g Ba3(PO4)2

5.00 g Ba3(PO4)2

1. Gas pressure is the result of …

2. What is STP (specifically)?

Day 5 11-14

Ideal gas

Kinetic-molecular Theory - Gases

– an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory

1520 mm Hg = ____ atms.

Use your notes to find the equivalence line.

Day 6 11-15