Effects of Increasing Temperature on Ideal Gas

[jimbo71]

Homework Statement

If you increase the temperature of an ideal gas, then
a. the average distance a molecule travels between collisions must increase
b. the pressure must increase
c. the speed of its molecules must increase
d. the average time between collisions of its molecule must increase
e. the volume must increase

Homework Equations

The Attempt at a Solution

I think the correct selection is choice C because while the other selections are possible only the energy is solely related to the temperature?

 

[aerospaceut10]

Yep. Kinetic-Molecular Theory and the calculation of the Root Mean Square velocity.

http://upload.wikimedia.org/math/e/e/1/ee164ebb93e704e4c8b5a781d6de2612.png

 

[thomate1]

Your answer is correct. As the temperature increases, the molecules in an ideal gas will have more kinetic energy, causing them to move faster. This will result in an increase in both the average distance traveled between collisions and the average time between collisions. However, the pressure and volume of an ideal gas are not solely dependent on temperature, as they are also affected by other factors such as the number of molecules and the size of the container. Therefore, choice C is the most accurate response to the statement.