Chemistry
Chapter 13 Study Questions
NOTE: Vapor
Pressure of Water Chart is on the back of this page.
1. A flask contains air at 722 mm Hg and 22°C. What would the temperature of the gas be if the pressure is increased to 1.07 atm?
2. A sample of air collected at STP contains 0.039 moles of N_{2}, 0.010 moles of O_{2}, and 0.001 moles of Ar. (Assume no other gases are present.)
a) Find the partial pressure of O_{2}.
b) What is the volume of the container?
3. A sample of hydrogen gas (H_{2}) is collected over water at 19°C.
a) What are the partial pressures of H_{2} and water vapor if the total pressure is 756 mm Hg?
b) What is the partial pressure of hydrogen gas in atmospheres?
4. If 600 cm^{3} of H_{2} at 25°C and 750 mm Hg is compressed to a volume of 480 cm^{3} at 41°C, what does the pressure become?
5. Find the density of helium gas at STP.
6. a) Write a balanced chemical equation for the reaction of butane gas with oxygen gas to form carbon dioxide and water vapor.
b) How many liters of oxygen are required to produce 2.0 liters of CO_{2}?
c) How many liters of CO_{2} are produced from 11.6 g of butane at STP?
d) How many molecules of water vapor are produced from 5.6 liters of butane gas at STP?
7. A flask contains 0.25 moles of argon and 0.75 moles of helium. If the partial pressure of the helium is 0.60 atm, what is the total pressure in the flask?
8. Calculate the density of carbon dioxide at 546 K and 4.00 atmospheres pressure.
9. How many grams of methane are contained in a 28.0 liter flask at 68°C and 2.00 atmospheres pressure?
10. What volume of O_{2} at 710 mm Hg pressure and 36°C is required to react with 6.52 g of CuS?
CuS(s) + 2 O_{2}(g) ® CuSO_{4}(s)
11. What is the molar mass of a gas if 7.00 grams occupy 6.20 liters at 29°C and 760 mm Hg pressure?
12. At a particular temperature and pressure, 15.0 g of CO_{2} occupy 7.16 liters. What is the volume of 12.0 g of CH_{4} at the same temperature and pressure?
Summary of Chapter 13: Gases
Kinetic-molecular theory
pressure
barometer, manometer
1 atm = 760 mmHg = 760 torr
temperature
absolute zero temperature
T(K) = T(°C) + 273
relationship between pressure, volume, temperature
Boyle’s Law
Charles’ Law
Avogadro's Law
Ideal Gas Law
R = 0.08206 L atm/mol K
partial pressure
molar volume
STP
molar volume @ STP = 22.4 L
gas stoichiometry
molar mass and density of a gas
formulas:
P_{total} = P_{x} + P_{y} + . . .
_{}
PV = nRT; R = 0.08206 L atm/mol K
d = _{}
_{}
Vapor Pressure of Water |
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Temp (°C) |
15 |
16 |
17 |
18 |
19 |
20 |
21 |
22 |
23 |
24 |
25 |
P_{H2O}(mm Hg) |
13 |
14 |
15 |
15 |
16 |
18 |
19 |
20 |
21 |
22 |
24 |