According to Gay-Lussac's law, how are pressure and temperature related?

Gay-Lussac's law states that for a given amount of gas at constant volume, the pressure of the gas is directly proportional to its absolute temperature (measured in Kelvin). This means that as the temperature increases, the pressure also increases, provided the volume does not change.

Mathematically, this relationship can be expressed as ( P \propto T ) when volume is constant, which indicates that if you double the temperature, the pressure will also double, reflecting that the two variables change in tandem. This principle is especially applicable in scenarios such as gas behavior in closed containers, where increases in temperature due to heat will result in increased molecular motion, causing more frequent and forceful collisions with the container walls, hence raising the pressure.

In contrast, the other options do not accurately describe the relationship outlined by Gay-Lussac's law. For example, stating that pressure is inversely proportional to temperature misunderstands this direct relationship. Similarly, claiming that pressure is unrelated to temperature ignores the significant influence temperature has on gas pressure. Lastly, mentioning that pressure depends on volume shifts the focus away from the core relationship between pressure and temperature defined by Gay-Lussac's law.