Dalton's Law of Partial Pressures



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Chemistry: Dalton’s Law of Partial Pressure

Directions: Solve each of the following problems. Show your work.

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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

O2 Ne H2S Ar Total

Moles 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 2) 5.0x102kPa 3) 812 mmHg 4) 2.41 L 5) 9.00

6) 1.20 atm 7) 704 mmHg 8) 83.7 kPa 9a) 15.0 mols 9b) 20.0 mols

9c) 35.0 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

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