1. a Student Collects Oxygen Gas by Water Displacement at a Temperature of 16 C. the Total

Dalton’s Law

Name: ______Date: ______

1.  A student collects oxygen gas by water displacement at a temperature of 16°C. The total volume is 188 ml at a pressure of 93.3 kPa. What is the pressure of the oxygen collected?

2.  A 0.540 L sample of hydrogen is collected over water at 12°C. The pressure of the hydrogen and water vapor mixture is 78.5 kPa. What is the partial pressure of the hydrogen gas?

3.  888 cm3 of carbon dioxide gas are collected over water at a temperature of 27°C. The total pressure of the gases is 55.8 kPa. What is the partial pressure of the dry gas?

Use the ideal gas law in combination with Dalton’s Law of partial pressures to solve the following problems:

4.  A sample of potassium chlorate is partially decomposed, producing oxygen gas that is collected over water. The volume of gas collected is 0.250 L at 26°C and 102.0 kPa total pressure.

a.  What is the pressure of the oxygen gas?

b.  How many moles of oxygen gas are collected?

c.  How many grams of oxygen gas are collected?

5.  Hydrogen gas is produced when zinc reacts with sulfuric acid. If 159 ml of wet hydrogen gas is collected over water at 24°C and 98.4 kPa, how many grams of hydrogen are collected?

Use Dalton’s relationship between moles and pressure to solve the following problems:

6.  What is the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mole of hydrogen and has a total pressure of 1.05 atm?

7.  Knowing that 2.0 moles of a gas can fill up a 32 L container, what number of moles would occupy 8.8 L at the same temperature and pressure?

8.  If 6.5 moles of helium occupy a volume of 250ml, what would the new volume be if 6.5 more moles of He were added?