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(D) The process described is free expansion of an ideal gas in an isolated chamber.For an ideal gas,internal energy $(U)$ is a function of temperature

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pressure

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(D) The process described is free expansion of an ideal gas in an isolated chamber.For an ideal gas,internal energy $(U)$ is a function of temperature $(T)$ only. Since the chamber is isolated,no heat $(q = 0)$ is exchanged with the surroundings,and since it is free expansion,no work is done $(w = 0)$.According to the first law of thermodynamics,$\Delta U = q + w = 0 + 0 = 0$.Since $\Delta U = 0$,the temperature $(T)$ remains constant.However,the volume $(V)$ of the gas increases from $V$ to $2V$.Using the ideal gas equation $PV = nRT$,since $n$,$R$,and $T$ are constant,$P$ is inversely proportional to $V$.As the volume doubles,the pressure $(P)$ must decrease to half of its initial value $(P_f = P/2)$.Therefore,the parameter that changes is pressure.

An isolated chamber is divided into two halves by a partition,with an ideal gas in one half. By making a hole in the partition,the gas is allowed to expand to the full chamber. Among the following,the parameter which changes in the process is

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