According to the kinetic molecular theory, what happens as the number of collisions of an ideal gas increases?

• A. The average kinetic energy of the gas molecules decreases.
• B. The temperature of the gas decreases.
• C. The volume of the gas must decrease.
• D. The pressure exerted by the gas increases.

Answer: (D)

Verified step by step guidance

1. Recall that according to the kinetic molecular theory, gas pressure is caused by collisions of gas molecules with the walls of the container.
2. Understand that the pressure exerted by a gas is directly related to the frequency and force of these molecular collisions.
3. Recognize that if the number of collisions increases, it means more molecules are hitting the container walls per unit time or with greater force.
4. Since pressure is defined as force per unit area, an increase in collisions leads to an increase in the force exerted on the container walls, thus increasing pressure.
5. Note that average kinetic energy and temperature are related, but an increase in collisions alone does not necessarily change the temperature or kinetic energy; it primarily affects pressure.