Dalton's Law of Partial Pressures
This worksheet covers Dalton's Law of Partial Pressures, including calculations and conceptual understanding for Grade 12 Chemistry students.
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Dalton's Law of Partial Pressures
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Read each question carefully and provide your answer in the space provided. Show all your work for calculation problems.
1. Dalton's Law of Partial Pressures states that the total pressure of a mixture of non-reacting gases is equal to the of the partial pressures of the individual gases.
2. The partial pressure of a gas is the pressure it would exert if it were the gas in the container.
3. The mole fraction of a gas in a mixture is defined as the ratio of the moles of that gas to the moles of all gases in the mixture.
1. A container holds a mixture of oxygen, nitrogen, and carbon dioxide. If the partial pressure of oxygen is 0.2 atm, nitrogen is 0.7 atm, and carbon dioxide is 0.1 atm, what is the total pressure in the container?
0.9 atm
1.0 atm
1.1 atm
1.8 atm
2. Which of the following conditions is necessary for Dalton's Law of Partial Pressures to apply?
The gases must be at different temperatures.
The gases must react with each other.
The gases must be non-reacting.
The gases must have different molar masses.
1. A gas mixture contains 4.0 moles of N2 and 1.0 mole of O2. If the total pressure of the mixture is 5.0 atm, what is the partial pressure of each gas?
2. Explain how Dalton's Law of Partial Pressures is applied in collecting gases over water.
1. If the temperature of a gas mixture increases, the partial pressure of each gas will decrease, assuming constant volume.
True
False
2. The mole fraction of a gas has no units.
True
False
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