Skip to ContentGo to accessibility pageKeyboard shortcuts menu
OpenStax Logo
College Physics for AP® Courses 2e

Test Prep for AP® Courses

College Physics for AP® Courses 2eTest Prep for AP® Courses

13.3 The Ideal Gas Law

1.

A fixed amount of ideal gas is kept in a container of fixed volume. The absolute pressure P, in pascals, of the gas is plotted as a function of its temperature T, in degrees Celsius. Which of the following are properties of a best fit curve to the data? Select two answers.

  1. Having a positive slope
  2. Passing through the origin
  3. Having zero pressure at a certain negative temperature
  4. Approaching zero pressure as temperature approaches infinity
2.
A black rectangle with bottom 2/3 grayed out and the word Gas shows. A thick solid black upside down T appears above the Gas area with the vertical part of the T extending past the edge of the box on the top. It is white inside the rectangle above the T at the top part of the rectangle.
Figure 13.34

This figure shows a clear plastic container with a movable piston that contains a fixed amount of gas. A group of students is asked to determine whether the gas is ideal. The students design and conduct an experiment. They measure the three quantities recorded in the data table below.

Trial Absolute Gas Pressure (x10m5 Pa) Volume (m3) Temp. (K)
11.10.020270
21.40.016270
31.90.012270
42.20.010270
52.80.008270
61.20.020290
71.50.016290
82.00.012290
92.40.010290
103.00.008290
111.30.020310
121.60.016310
132.10.012310
142.60.010310
153.20.008310
Table 13.6
  1. Select a set of data points from the table and plot those points on a graph to determine whether the gas exhibits properties of an ideal gas. Fill in blank columns in the table for any quantities you graph other than the given data. Label the axes and indicate the scale for each. Draw a best-fit line or curve through your data points.
  2. Indicate whether the gas exhibits properties of an ideal gas, and explain what characteristic of your graph provides the evidence.
  3. The students repeat their experiment with an identical container that contains half as much gas. They take data for the same values of volume and temperature as in the table. Would the new data result in a different conclusion about whether the gas is ideal? Justify your answer in terms of interactions between the molecules of the gas and the container walls.

13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature

3.

Two samples of ideal gas in separate containers have the same number of molecules and the same temperature, but the molecular mass of gas X is greater than that of gas Y. Which of the following correctly compares the average speed of the molecules of the gases and the average force the gases exert on their respective containers?

Average Speed of MoleculesAverage Force on Container
(a)Greater for gas XGreater for gas X
(b)Greater for gas XThe forces cannot be compared without knowing the volumes of the gases.
(c)Greater for gas YGreater for gas Y
(d)Greater for gas YThe forces cannot be compared without knowing the volumes of the gases.
Table 13.7
4.

How will the average kinetic energy of a gas molecule change if its temperature is increased from 20ºC to 313ºC?

  1. It will become sixteen times its original value.
  2. It will become four times its original value
  3. It will become double its original value
  4. It will remain unchanged.
5.
The graph shows a vertical, y-axis labeled Probability and a horizontal, x-axis labeled velocity v (m over s). There are two distribution curves, a red one marked T1 and a green one labeled T2. The red curve rises quickly and the gradually tapers off. The green curve rises slower than the red curve (and thus is to the right of the red curve), peaks lower than the peak of the red curve and then tapers down less quickly than the red curve.
Figure 13.35

This graph shows the Maxwell-Boltzmann distribution of molecular speeds in an ideal gas for two temperatures, T1 and T2. Which of the following statements is false?

  1. T1 is lower than T2
  2. The rms speed at T1 is higher than that at T2.
  3. The peak of each graph shows the most probable speed at the corresponding temperature.
  4. None of the above.
6.

Suppose you have gas in a cylinder with a movable piston which has an area of 0.40 m2. The pressure of the gas is 150 Pa when the height of the piston is 0.02 m. Find the force exerted by the gas on the piston. How does this force change if the piston is moved to a height of 0.03 m? Assume temperature remains constant.

7.

What is the average kinetic energy of a nitrogen molecule (N2) if its rms speed is 560 m/s? At what temperature is this rms speed achieved?

8.

What will be the ratio of kinetic energies and rms speeds of a nitrogen molecule and a helium atom at the same temperature?

PreviousNext
Order a print copy
Citation/Attribution

This book may not be used in the training of large language models or otherwise be ingested into large language models or generative AI offerings without OpenStax's permission.

Want to cite, share, or modify this book? This book uses the Creative Commons Attribution License and you must attribute OpenStax.

Attribution information
  • If you are redistributing all or part of this book in a print format, then you must include on every physical page the following attribution:
    Access for free at https://openstax.org/books/college-physics-ap-courses-2e/pages/1-connection-for-ap-r-courses
  • If you are redistributing all or part of this book in a digital format, then you must include on every digital page view the following attribution:
    Access for free at https://openstax.org/books/college-physics-ap-courses-2e/pages/1-connection-for-ap-r-courses
Citation information

© Jul 9, 2024 OpenStax. Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License . The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo are not subject to the Creative Commons license and may not be reproduced without the prior and express written consent of Rice University.