Increasing the temperature of a gas increases the kinetic energy of its particles, causing them to move faster. With higher speeds, gas particles collide more frequently and with greater force, resulting in an increase in the pressure exerted by the gas on the walls of the container.
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Increasing the temperature of a gas increases the average kinetic energy of its molecules, causing them to move faster and collide with the container walls more frequently and with greater force. These collisions exert a higher pressure on the container, as described by the kinetic theory of gases. Thus, temperature and pressure are directly proportional in accordance with the ideal gas law.
Increasing the temperature of a gas increases its pressure because of the relationship between temperature, kinetic energy, and the motion of gas particles. When the temperature of a gas rises, the kinetic energy of its particles also increases. As a result, the gas particles move faster and collide with the walls of their container more frequently and with greater force.
The increased frequency and intensity of these collisions generate higher pressure inside the container. According to the ideal gas law (PV = nRT), an increase in temperature (T) at constant volume (V) and a fixed amount of gas (n) leads to an increase in pressure (P). Therefore, higher temperatures result in higher gas pressure due to the increased kinetic energy and speed of the gas particles, causing them to exert more force on their container’s walls.