Revised: 2021-03-18
Answers: 12) a. 0.295 mol, b. 0.595 g 13) 3.29 atm 14) 3760 K 15) 36.2 L 16) 5040 L, 3.47x10-4 g/L 17) 24.8 L 18) 6.16 g Na 19) 5.00 atm 20) 0.28 L
Name:
Date: Per:
Chapter 11
Practice Test
Kinetic Molecular Theory
1. List the five postulates of the Kinetic-Molecular Theory.
Name the Gas Law
2. A potato chip bag pops when taken up in the mountains.
3. A balloon put in the freezer shrinks.
4. A lighter gas moves faster than a heavier gas.
5. The pressure of two gases is the sum of their partial pressures.
Calculations, Etc.
6. Equal amounts of gas at the same temperature and pressure have the same .
7. If the temperature of a sample of gas is halved at constant volume, the pressure will be .
8. The temperature at which matter stops moving is called .
9. The values of standard temperature are .
10. The values of standard pressure (in atm & mmHg) are .
11. Derive the value of R for pressure in atmospheres. (Must show work)
How would this process be different if you were to calculate the value of R for mmHg?
12. A sample of hydrogen gas has a volume of 4.40 L at a temperature of 145 °C and a pressure of 2.30 atm.
a) How many moles are in the sample?
V = 4.40 L
PV = nRT
T = 145 ℃ (418 K)
P = 2.30 atm
n =
PV
=
(2.30 atm)(4.40 L)
= 0.2948 mol 0.295 mol H2
n = ?
RT
(0.0821 (atm•L)/(mol•K))(418 K)
R = 0.0821 (atm•L)/(mol•K)
b) What is the mass of the sample?
0.2948 mol H2
2.018 g H2
= 0.5943 g 0.594 g H2
1 mol H2
13. A sample of gas measures 5.00 liters at 2.30 atmospheres of pressure. To change the volume to 3.50 liters at constant
temperature, what pressure must be applied?
V1 = 5.00 L
P1V1 = P2V2
P1 = 2.30 atm
V2 = 3.50 L
P2 =
P1V1
=
(2.30 atm)(5.00 L)
= 3.2857 atm 3.29 atm
P2 = ?
V2
(3.50 L)
