If you double the absolute temperature of a gas while keeping its pressure constant, what happens to its volume?

When the absolute temperature of a gas is doubled while keeping its pressure constant, the volume of the gas also doubles. This relationship is explained by Charles's Law, which states that the volume of a gas is directly proportional to its absolute temperature when the pressure is held constant. In mathematical terms, this is expressed as V/T = k, where V is volume, T is temperature in Kelvin, and k is a constant for a given amount of gas at constant pressure.

By doubling the temperature (T), the equation can be rearranged to show that if V is directly proportional to T, then when T increases to 2T, V must also increase to 2V in order to maintain the equality. Thus, at constant pressure, an increase in temperature results in a proportional increase in volume, confirming that the volume doubles as the temperature doubles.