Name: _______________________
Class________________
Chemistry: Dalton’s Law of Partial Pressure
Directions: Solve each of the following problems. Show your work.
1. Container A (with volume 1.23 dm3) contains a gas under 3.24 atm of pressure. Container B
(with volume 0.93 dm3) contains a gas under 2.82 atm of pressure. Container C (with
volume 1.42 dm3) contains a gas under 1.21 atm of pressure. If all of these gases are put
into Container D (with volume 1.51 dm3), what is the pressure in Container D?
2. Container A (with volume 1.56 L) contains a gas under 185.3 kPa of pressure. Container B has
1
/3 the volume of Container A, but its gas is under twice the pressure as that of
Container A. If the gases from A and B are combined into Container C (with volume 0.95
L), what is the pressure in Container C?
3. Container A (with volume 150 mL) contains a gas under an unknown pressure. Container B
(with volume 250 mL) contains a gas under 628 mm Hg of pressure. Container C (with
volume 350 mL) contains a gas under 437 mm Hg of pressure. If all of these gases are
put into Container D (with volume 300 mL),, giving it 1439 mm Hg of pressure, find the
original pressure of the gas in Container A.
4. The gases of three identical containers A, B, and C are under pressures of 1.44 atm, 3.16
atm, and 2.52 atm, respectively. These gases are then combined into Container D (with a
volume of 3.92 L) so that the pressure in Container D is 4.38 atm. Containers A, B, and C
have the same volume. Find that volume.
5. A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of
the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure
inside the container?
6. A container with two gases, helium and argon, is 30.0% by volume helium. Calculate the partial
pressure of helium and argon if the total pressure inside the container is 4.00 atm.
7. If 60.0 L of nitrogen is collected over water at 40.0 °C when the atmospheric pressure is
760.0 mm Hg, what is the partial pressure of the nitrogen?
8. 80.0 liters of oxygen is collected over water at 50.0 °C. The atmospheric pressure in the
room is 96.00 kPa. What is the partial pressure of the oxygen?
9. A tank contains 480.0 grams of oxygen and 80.00 grams of helium at a total pressure of 7.00
atmospheres. Calculate the following.
a) How many moles of O2 are in the tank?
b) How many moles of He are in the tank?
c) Total moles of gas in tank.
d) Mole fraction of O2.
e) Mole fraction of He.
f) Partial pressure of O2.
g) Partial pressure of He.
10. A tank contains 5.00 moles of O2, 3.00 moles of neon, 6.00 moles of H2S, and 4.00 moles of
argon at a total pressure of 1620.0 mm Hg. Complete the following table
Moles
O2
Ne
H2S
Ar
Total
18.00
Mole fraction
1
Pressure fraction
1
Partial Pressure
1620.0
11. A mixture of 14.0 grams of hydrogen, 84.0 grams of nitrogen, and 2.0 moles of oxygen are
placed in a flask. When the partial pressure of the oxygen is 78.00 mm of mercury, what is the
total pressure in the flask?
12. A flask contains 2.00 moles of nitrogen and 2.00 moles of helium. How many grams of argon
must be pumped into the flask in order to make the partial pressure of argon twice that of
helium?
Ans:
1) 5.5 atm
6) 1.20 atm
9c) 35.0 mols
2) 5.0x102kPa
3) 812 mmHg
4) 2.41 L
5) 9.00
7) 704 mmHg
8) 83.7 kPa 9a) 15.0 mols
9b) 20.0 mols
9d) 0.429
9e) 0.571
9f) 3.00 atm
9g) 4.00 atm
10) moles: 5.00; 3.00; 6.00; 4.00
Mole fraction: 0.278; 0.167; 0.333; 0.222
Pressure fraction: 0.278; 0.167; 0.333; 0.222
Partial pressure (mmHg): 450.; 271; 539; 360.
11) 464 mmHg
12) 160. g Ar