Pressure is the force exerted per unit area. In gases, it arises from the collisions of gas molecules with the walls of the container.

Temperature is a measure of the average kinetic energy of the molecules within a substance. Higher temperature means higher average kinetic energy.

Kinetic energy is the energy an object possesses due to its motion. It is directly proportional to the mass and the square of the velocity of the object.

An ideal gas is a theoretical gas composed of randomly moving point particles that do not interact except when they collide elastically.

Average kinetic energy is directly proportional to the absolute temperature of the gas. An increase in temperature results in a proportional increase in the average kinetic energy of the gas molecules.

Increasing the temperature increases the average kinetic energy of the gas molecules, leading to more frequent and forceful collisions with the container walls, thus increasing the pressure.

The collisions exert a force on the walls. The sum of these forces over the area of the walls determines the pressure exerted by the gas.

Decreasing the volume increases the frequency of collisions of gas molecules with the container walls, resulting in an increase in pressure.

An increase in the average speed of gas molecules leads to a higher average kinetic energy, resulting in an increase in temperature and a potential increase in pressure if the volume is constant.

Adding more gas molecules increases the number of collisions with the container walls, resulting in an increase in pressure, assuming volume and temperature are constant.

The average speed of the gas atoms increases, leading to more frequent and forceful collisions with the container walls, which increases pressure.

The pressure of the gas increases because the atoms collide more frequently with the container walls.

The temperature of the gas increases.

An increase in pressure.

Cooling a gas slows down the atoms, decreasing their kinetic energy and the temperature.