An ideal gas is enclosed in a container. The volume of the container is reduced to half the original volume at constant temperature. According to kinetic theory, what is the best explanation for the increase in pressure created by the gas?

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The average speed of the gas particles is unchanged, but they hit the container walls more frequently

The average speed of the gas particles increases as does the frequency with which they hit the container walls.

The average speed of the gas particles increases, overcoming the decreased frequency that they hit the container walls.

The average speed of the gas particles decreases, but they hit the container walls more frequently

answer is B.

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Detailed Solution

The average speed of molecules (rms-speed effectively) is dependent on temperature. A particle has to travel in order to collide with the walls of the container is greatly decreased... hence there is an increase in the frequency with which particles hit the wall. This is reason for the pressure increase.

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