Final answer:
The statement is True because as the temperature of a gas increases, so does the average kinetic energy of its particles, causing faster and more forceful collisions with the container walls. This principle is supported by the kinetic molecular theory and Amontons's law.
Step-by-step explanation:
As a gas is heated, the temperature increases and so does the average kinetic energy of the particles in the gas. This is because the temperature of gases is proportional to the average translational kinetic energy of atoms and molecules. When the kinetic energy increases, the particles move faster, resulting in more forceful impacts with the walls of the container.
According to Amontons's law, an increase in temperature, while keeping the volume constant, leads to an increase in the speed and kinetic energy of gas molecules. This causes more frequent and forceful collisions with the container's walls, thus increasing the pressure.