Name: _____________________________ Period: ______
Gas Laws Worksheet #6 – Dalton’s Law of Partial Pressures
1. Consider the following apparatus: Two glass spheres, one filled with nitrogen and the other filled with oxygen are
connected by a tube with a valve in the middle. The sphere with nitrogen has 2 liters, at 1 atm and 25C. The sphere
with oxygen contains 3 L, at 2.0 atm, at 25C. When the valve between the two containers is opened, the gasses are
allowed to mix. What is the partial pressure of the nitrogen, what is the partial pressure of the oxygen, and what is the
total pressure?
2. A mixture containing 0.538 mol He, 0.315 mol Ne, and 0.103 mol Ar is confined in a 7.00 L vessel at 25C.
a. Calculate the partial pressure of each of the gases in the mixture in atm
b. Calculate the total pressure of the mixture
3. A mixture containing 2.50 g each of CH4, C2H4, and C4H10 is contained in a 1.50L flask at a temperature of 15C
a. Calculate the partial pressure of each of the gases in the mixture in atm
b. Calculate the total pressure of the mixture
4. A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2 in a 3.5L container at 80C.
a. Calculate the partial pressure of each of the gases in the mixture in atm
b. Calculate the total pressure of the mixture
5. A mixture of gases contains 5.10g of N2, 2.93 g of H2, and 5.17 g of NH3. If it is being confined in a 13.4 L container
at 120C.
a. Calculate the partial pressure of each of the gases in the mixture in atm
b. Calculate the total pressure of the mixture
6. What is the pressure in atm of a gas mixture that contains 1.0 g of H2 and 8.0 g of Ar in a 3.0 L container at 27C?
7. Two tanks are connected by a closed valve. Each tank is filled with gas, and both tanks are held at the same
temperature. We open the valve and allow the gases to mix. Tank A contains 5.00 L of oxygen at 24 atm, and tank B
contains 3L of nitrogen at 32.0 atm.
a. After the gases mix, what is the partial pressure of each gas?
b. What is the total pressure?
8. A gaseous mixture contains 3.23 g of chloroform, CHCl3, and 1.22 g of methane, CH4. Assuming that both compounds
remain as gases, what pressure is exerted by the mixture inside a 50.0 ml metal container at 275C? What is each of the
partial pressures in atm?
9. One container with a volume of 1.00 L contains argon at a pressure of 1.77 atm, and a second container of 1.50 L
volume contains argon at a pressure of .487 atm. They are then connected to each other so that the pressure can
become equal in both containers.
a. What is the partial pressure of each gas?
b. What is the total pressure?
10. Mixtures of helium and oxygen can be used in scuba diving tanks to help prevent “the bends.” For a particular dive,
46L of He at 25C and 1.0 atm and 12L of O2 at 25C and 1.0 atm were pumped into a 5.0L tank.
a. What is the partial pressure of each gas?
b. What is the total pressure?
11. A mixture of 1.00 g of H2and 1.00g of He is placed in a 1.00L container at 27C. Calculate the partial pressure of each
gas and the total pressure in atm.
12. A 10.0L flask at 27C contains 6.0grams of H2, 15.2g of N2, and 16.8g of He.
a. Calculate the partial pressure of each gas in atm.
b.
What is the total pressure?