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Holt Chemistry Chapter 12: Gases Chapter Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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Question 1 1. If carbon dioxide molecules effuse at an average rate of 5 mol/s, at what rate would diatomic hydrogen molecules effuse in the exact same conditions?

Question 2 2. What does the Maxwell-Boltzmann curve tell us?

Question 3 3. Why can't all of the gas particles in a container have very high or very low speeds?

Question 4 4. If someone is measuring pressure, they might use any of the following units EXCEPT _____.

Question 5 5. 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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Question 6 6. At constant temperature, what happens to the pressure when the volume is doubled?

Question 7 7. To use Gay-Lussac's Law, which of the following needs to remain constant?

Question 8 8. Dana has placed a few drops of food coloring in a mixture of water and vinegar to dye hard-boiled eggs with her daughter in preparation for Easter. The food coloring changing the color of the water is an example of _____.

Question 9 9. Which of the following is TRUE about ideal gas particles?

Question 10 10. If a 22.4 L container is holding 1.00 mole of a gas at 273 kelvins, then what is its pressure?

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Question 11 11. A 4 L sample of gas is heated from 20 K to 200 K. What will its final volume be?

Question 12 12. What volume is occupied by 15.0 moles of carbon dioxide gas at standard temperature and pressure?

Question 13 13. Why does the probability curve become narrower when gas particles are more massive?

Question 14 14. How does a higher temperature affect the probability distribution curve of gas particles?

Question 15 15. According to the kinetic molecular theory, temperature is directly proportional to _____.

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Question 16 16. Hugo measures the pressure in his car's tire and finds that it is 32 Psi. What is the pressure if he converts this measurement from Psi to Torr?

Question 17 17. The _____ states that gas particles are constantly moving in rapid, random movement.

Question 18 18. Mark has unknowingly driven over a very large nail when exiting his work parking lot. He has a long commute home, and by the time he arrives he will have a flat tire. The air that is slowly escaping from the hole in his tire is an example of _____.

Question 19 19. The ideal gas constant, R, can be found using which of the following equations?

Question 20 20. Assuming the volume is held constant, what happens to the pressure of a gas when the absolute temperature doubles?

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Question 21 21. Which of the following is TRUE about most gases?

Question 22 22. A container has a volume of 53.9 L. Assuming it is at STP, how many moles of gas particles does it contain?

Question 23 23. Which of the following statements best represents Graham's Law?

Question 24 24. A 4 L sample of gas is heated from 20 K to 200 K. Its initial pressure was 60 torr. What is its final pressure?

Question 25 25. Which of the following is the best definition for Torr?

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Question 26 26. Assuming pressure and temperature are held constant, then what happens to the volume of a non-rigid container when the number of molecules in the container is doubled?

Question 27 27. 1000 mL of a gas at 15 atm is compressed to 500 mL. What is its new pressure?

Question 28 28. Which of the following actions would cause an individual to experience lower pressure as measured in Atmospheres?

Question 29 29. If you know the temperature, volume, and pressure of a gas, how would you rearrange the ideal gas equation to find the number of moles?

Question 30 30. A gas is collected by water displacement at 25 degrees Celsius. The vapor pressure of water at that temperature is 24 mmHg. If the atmospheric pressure is 800 mmHg, then what is the pressure of the dry gas you collected?

Holt Chemistry Chapter 12: Gases Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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