What does the Universal Gas Law state about the relationship between pressure and temperature?

The Universal Gas Law, often represented by the equation PV = nRT, describes the relationships between pressure (P), volume (V), temperature (T), and the number of moles of a gas (n) at a constant amount of gas. When we isolate the relationship between pressure and temperature, while assuming volume remains constant, we can derive that pressure is directly proportional to temperature.

This means that as the temperature of a gas increases, the kinetic energy of the gas molecules also increases, causing them to collide with the walls of their container more forcefully and more frequently. Consequently, the pressure exerted by the gas will increase with a rise in temperature.

This direct relationship is a result of the assumptions made in the ideal gas law and is fundamental in understanding how gases behave under varying conditions. If the volume is held constant, it becomes evident that for an ideal gas, doubling the temperature (in Kelvin) while keeping the volume constant would also double the pressure, thereby illustrating this direct connection.