What is the effect of temperature on gas pressure in a closed container?

In a closed container, the relationship between temperature and gas pressure is directly proportional, meaning that as the temperature increases, the gas pressure also increases. This behavior is explained by the kinetic molecular theory, which states that gas particles move more rapidly when heated. As the temperature rises, the average kinetic energy of the gas molecules increases, causing them to collide with the walls of the container more frequently and with greater force. These more frequent and energetic collisions lead to an increase in pressure within the container.

When considering the other options, decreasing pressure with temperature fails to align with established gas laws, such as Gay-Lussac's law, which states that pressure and temperature are directly related when volume is constant. The idea of no effect on pressure contradicts the fundamental principles governing gas behavior, as external conditions, including temperature, consistently influence gas pressure. The notion of negative pressure is not feasible in typical physical scenarios, as pressure is a measure of force applied over an area and cannot be negative under standard conditions. Thus, the understanding that pressure increases with temperature is a well-supported concept in thermodynamics and gas behavior.