Dalton's Law of Partial Pressures
Explore Dalton's Law of Partial Pressures with this worksheet, covering gas mixtures, partial pressures, and mole fractions through various question types.
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Dalton's Law of Partial Pressures Worksheet
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Read each question carefully and answer to the best of your ability. Show all work for calculations.
1. Which of the following statements best describes Dalton's Law of Partial Pressures?
The total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases.
The pressure of a gas is inversely proportional to its volume at constant temperature.
The volume of a gas is directly proportional to its absolute temperature at constant pressure.
The rate of effusion of a gas is inversely proportional to the square root of its molar mass.
2. A container holds a mixture of oxygen (O₂) and nitrogen (N₂). If the partial pressure of O₂ is 0.4 atm and the total pressure is 1.2 atm, what is the partial pressure of N₂?
0.4 atm
0.8 atm
1.2 atm
1.6 atm
3. 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.
4. The partial pressure of a gas in a mixture is the pressure that gas would exert if it were in the container.
5. According to Dalton's Law, the partial pressure of a gas is independent of the other gases present in the mixture.
True
False
6. Dalton's Law applies to ideal gases and is less accurate for real gases at high pressures or low temperatures.
True
False
7. A mixture of gases contains 2.0 moles of O₂, 3.0 moles of N₂, and 1.0 mole of CO₂. If the total pressure of the mixture is 6.0 atm, what is the partial pressure of each gas?
8. Explain why Dalton's Law of Partial Pressures is useful in understanding the composition of air.