How does the pressure of an enclosed gas in a rigid container change when the gas is heated?

The observed behavior of gas in a rigid container when heated aligns with the principles described by the kinetic molecular theory and the ideal gas law. When a gas is heated, its temperature increases, which results in the gas particles gaining kinetic energy. This increase in kinetic energy causes the particles to move faster and collide with the walls of the container more frequently and with greater force.

Since the container is rigid, it does not allow for any change in volume. Therefore, as the speed of the gas particles increases, the number of collisions against the walls of the container increases, which directly leads to an increase in pressure. The relationship can be described by Gay-Lussac's Law, which states that for a given mass of gas at constant volume, the pressure is directly proportional to the temperature (in Kelvin).

Thus, in a rigid container, heating the gas will invariably result in an increase in pressure due to the increased motion of the particles.