What happens when temperature increases in a confined gas with no room to expand?

When the temperature of a confined gas increases and there is no room for expansion, the kinetic energy of the gas molecules also increases. As the molecules move faster, they collide with the walls of their container more frequently and with greater force. This increased frequency and energy of collisions result in an increase in pressure within the confined space.

According to Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume is held constant, this scenario directly applies. If the volume cannot change and the temperature rises, the pressure must rise as well.

If the pressure exceeds the strength of the container, it can potentially lead to failure, such as bursting or rupture of the container due to the extreme internal pressure. Therefore, understanding the relationship between temperature and pressure in a confined gas helps emphasize the potential dangers of increasing temperatures without any means of expansion. This context explains why the correct answer highlights the increase in pressure and the risk of failure.