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Dalton's Law of Partial Pressures: Calculating Partial & Total Pressures

Instructions:

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question 1 of 3

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

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1. A gaseous mixture contains 5.0 moles of nitrogen and 10.0 moles of helium. The total pressure in the container is 3 atmospheres. What is the partial pressure of the nitrogen?

2. A sealed vessel contains 0.5 moles of oxygen, 0.1 moles of carbon dioxide, and 0.4 moles of nitrogen gas. The total pressure of the gas mixture is 5 atmospheres. What is the partial pressure of the carbon dioxide?

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About This Quiz & Worksheet

The following quiz and worksheet combo will check your understanding of Dalton's Law of Partial Pressures.

Quiz & Worksheet Goals

During the assessments, you will be tested on:

  • Partial pressure of carbon dioxide
  • Pressure of dry gas
  • Partial pressure of nitrogen
  • Atmospheric pressure

Skills Practiced

  • Information recall - access the knowledge you've gained regarding Dalton's Law of Partial Pressures
  • Knowledge application - use your knowledge to answer questions about gas mixtures
  • Defining key concepts - ensure that you can accurately define key terms, such as total and partial pressure

Additional Learning

To learn more about Dalton's influence on the study of gas, review the accompanying lesson called Dalton's Law of Partial Pressures: Calculating Partial & Total Pressures. With this lesson, you can meet the following objectives:

  • Detail gas mixtures
  • Define partial pressure of a gas
  • Explain collecting gas over water
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