If both the volume and the absolute temperature of a confined gas are doubled, what will happen to the pressure?

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When both the volume and the absolute temperature of a confined gas are doubled, according to the ideal gas law (PV = nRT), the pressure remains unchanged under these conditions.

In the ideal gas law, P represents pressure, V represents volume, T represents absolute temperature, and n is the number of moles of gas along with R, which is the ideal gas constant. When you double the volume (V) of a gas and simultaneously double its absolute temperature (T), the changes effectively balance each other out.

To illustrate this, if you start with an initial state of the gas at pressure P, volume V, and temperature T, after doubling the volume to 2V and the temperature to 2T, the equation can be reconsidered. Since pressure is inversely related to volume and directly related to temperature, these two changes counteract each other, resulting in no net change in pressure.

This balance demonstrates why the pressure of the gas remains constant, affirming that the correct answer to the question is that the pressure will remain unchanged.

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