Pressure and temperature have which kind of relationship?

The relationship between pressure and temperature in an ideal gas is a direct one, which means that as the temperature increases, the pressure also increases, assuming the volume remains constant. This direct relationship is articulated in Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature (measured in Kelvin) when the volume is kept constant.

In mathematical terms, this can be expressed as P/T = constant, where P represents the pressure and T represents the temperature. Therefore, if you increase the temperature of a gas, the kinetic energy of the gas molecules increases, leading to more frequent and forceful collisions with the walls of the container, which results in an increase in pressure.

Understanding this direct relationship is crucial for solving problems related to gas behavior under varying conditions of temperature and pressure, and it reinforces the principle that manipulation of one parameter will directly affect the other in a predictable manner for an ideal gas.