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Which of the following statements best explains what happens if you increase the temperature of a gas inside a glass container? If the container is rigid the volume of the container does not change (that is, the volume is constant). Since the volume of the gas does not change, Boyle's Law tells us that the pressure of the gas will also not change because the equation P1V1 = P2V2 does not depend on temperature. As you increase the temperature of the gas, the gas particles expand in size. O Since each particle now occupies a larger volume, this means the total gas also occupies a larger volume, which in turn increases the pressure. As the temperature increases you are increasing the kinetic energy of the gas particles. As the gas particles move faster, they are more likely to collide with the walls of the container. This increase in the number of collisions causes an increase in the pressure of the gas. As you increase the temperature of the gas the container itself will expand, causing the volume to increase. The larger volume of the container means the gas particles have more space in which to move, which reduces the number of collisions. Fewer collisions results in a lower pressure of the gas.

Which of the following statements best explains what happens if you increase the temperature of a gas inside a glass container? If the container is rigid the volume of the container does not change (that is, the volume is constant). Since the volume of the gas does not change, Boyle's Law tells us that the pressure of the gas will also not change because the equation P1V1 = P2V2 does not depend on temperature. As you increase the temperature of the gas, the gas particles expand in size. O Since each particle now occupies a larger volume, this means the total gas also occupies a larger volume, which in turn increases the pressure. As the temperature increases you are increasing the kinetic energy of the gas particles. As the gas particles move faster, they are more likely to collide with the walls of the container. This increase in the number of collisions causes an increase in the pressure of the gas. As you increase the temperature of the gas the container itself will expand, causing the volume to increase. The larger volume of the container means the gas particles have more space in which to move, which reduces the number of collisions. Fewer collisions results in a lower pressure of the gas.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A mixture of three gases has a total pressure of 5 atm. If the partial pressure of the first gas is 3 atm, and the partial pressure of the second gas is 1.5 atm, what is the partial pressure of the third gas? You cannot know the partial pressure of the third gas without knowing the temperature of the gas mixture 02 atm 01 atm O 0.5 atm
Transcribed Image Text:A mixture of three gases has a total pressure of 5 atm. If the partial pressure of the first gas is 3 atm, and the partial pressure of the second gas is 1.5 atm, what is the partial pressure of the third gas? You cannot know the partial pressure of the third gas without knowing the temperature of the gas mixture 02 atm 01 atm O 0.5 atm
Which of the following statements best explains what happens if you increase the temperature of a gas inside a glass container? If the container is rigid the volume of the container does not change (that is, the volume is constant). Since the volume of the gas does not change, Boyle's Law tells us that the pressure of the gas will also not change because the equation P1V1 = P2V2 does not depend on temperature. As you increase the temperature of the gas, the gas particles expand in size. O Since each particle now occupies a larger volume, this means the total gas also occupies a larger volume, which in turn increases the pressure. As the temperature increases you are increasing the kinetic energy of the gas particles. As the gas particles move faster, they are more likely to collide with the walls of the container. This increase in the number of collisions causes an increase in the pressure of the gas. As you increase the temperature of the gas the container itself will expand, causing the volume to increase. The larger volume of the container means the gas particles have more space in which to move, which reduces the number of collisions. Fewer collisions results in a lower pressure of the gas.
Transcribed Image Text:Which of the following statements best explains what happens if you increase the temperature of a gas inside a glass container? If the container is rigid the volume of the container does not change (that is, the volume is constant). Since the volume of the gas does not change, Boyle's Law tells us that the pressure of the gas will also not change because the equation P1V1 = P2V2 does not depend on temperature. As you increase the temperature of the gas, the gas particles expand in size. O Since each particle now occupies a larger volume, this means the total gas also occupies a larger volume, which in turn increases the pressure. As the temperature increases you are increasing the kinetic energy of the gas particles. As the gas particles move faster, they are more likely to collide with the walls of the container. This increase in the number of collisions causes an increase in the pressure of the gas. As you increase the temperature of the gas the container itself will expand, causing the volume to increase. The larger volume of the container means the gas particles have more space in which to move, which reduces the number of collisions. Fewer collisions results in a lower pressure of the gas.
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