Question

If you want to study the relationship between temperature and pressure of a gas, which factor must be held constant?

Answer 1

The temperature at a given volume and the pressure of a given amount of gas are directly proportional. Pressure rises when a system's temperature rises, and vice versa. The Gay-Lussac law describes the connection between a gas's pressure and temperature.

Complete step by step answer:
When it comes to gases, the link between pressure and temperature is described. The gas law that describes the pressure-temperature relationship is Gay-law. It asserts that the pressure of a given amount of a particular gas is precisely proportional to its Kelvin temperature at a constant volume. It's possible to write it as:
$P\,\,\propto \,\,T$ or,
$\dfrac{P}{T} = k$ (Where, $k$ is the constant)
If we want to compare a gas's temperature or pressure after changing one of its variables, we can use the following equation:
$\dfrac{{{P_1}}}{{{T_1}}} = \dfrac{{{P_2}}}{{{T_2}}}$
${P_1},{P_2}\;$ are the pressures of the two gases
${T_1},{T_2}\;$ are the temperatures of the two gases
When the temperature of a system is raised, the molecules in the gas travel quicker, increasing the pressure on the gas container's wall. This, in turn, raises the system's pressure. The pressure decreases as the system's temperature decreases. As a result, the pressure of a specific gas is precisely proportional to its temperature at a constant volume.

Note: It's worth mentioning that this equation holds true since temperature is a measure of a substance's average kinetic energy; as a gas's kinetic energy rises, its particles hit the container walls more quickly, increasing pressure.