Use the kinetic–molecular theory to explain why gas pressure increases if the temperature is raised and the volume is kept constant.

Question

Accepted Answer

Hello. And this problem were asked based on the kinetic molecular theory, which of the following statements best explains the increase in gas pressure as the temperature has increased a constant volume. Looking at it says the gas pressure increases as temperature increases a constant volume because gas particles exhibit elastic collisions. And this is true that that means that the kinetic energy all goes to increase the gas pressure. The next one says the gas pressure increases as the temperature increases at constant volume because gas particles have kinetic energy proportional to Kelvin temperature. This is also true. So as the temperature increases, average kinetic energy increases, this then results in an increase in the force per unit area, this results then in a increase in the pressure exerted by the gas on the walls of its container. And see says the gas pressure increases as the temperature increases at constant volume because gas particles can be compressed without gas molecule interactions. This is also true. So the volume of gas particles is less than the volume between particles which says then that they can be compressed without the molecules interacting. So A B and C are all explanations for why increase in gas pressure is associated with the temperature increase at constant volume. So the correct answer then is D all of the above. Thanks for watching. Hope.

Use the kinetic–molecular theory to explain why gas pressure increases if the temperature is raised and the volume is kept constant.

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Key Concepts

Kinetic-Molecular Theory

Gas Pressure

Charles's Law