Questions: When the temperature of a gas is increased within a closed container, pressure increases due to which of the following? A The gas turns into a liquid. B The frequency of collisions between molecules and the container walls decreases. C The frequency of collisions between molecules and the container walls increases. D The spaces between the molecules of gas decrease.

Solution Steps

In a closed container, when the temperature of a gas is increased, the kinetic energy of the gas molecules also increases. This is because temperature is a measure of the average kinetic energy of the molecules in a substance.

As the kinetic energy of the gas molecules increases, the molecules move faster. This increased speed results in more frequent collisions with the walls of the container. According to the kinetic molecular theory, the pressure exerted by a gas is due to these collisions.

Given the options:

• A: The gas turns into a liquid. (This is incorrect as increasing temperature generally does not cause a gas to liquefy.)
• B: The frequency of collisions between molecules and the container walls decreases. (This is incorrect because increased temperature increases collision frequency.)
• C: The frequency of collisions between molecules and the container walls increases. (This is correct as explained above.)
• D: The spaces between the molecules of gas decrease. (This is incorrect; while the average distance between molecules may change, it is not the primary reason for increased pressure.)

Final Answer