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(A) For an ideal gas,the work done in an expansion process is related to the number of moles $n$ by the ideal gas equation $pV = nRT$. Since $p$,$V$,a

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$NH_{3}$

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(A) For an ideal gas,the work done in an expansion process is related to the number of moles $n$ by the ideal gas equation $pV = nRT$. Since $p$,$V$,and $T$ are constant,$n$ must be constant for all gases. Given that the mass $m$ of each gas is the same,the number of moles is given by $n = \frac{m}{M}$,where $M$ is the molar mass. For $n$ to be constant for a fixed mass $m$,the molar mass $M$ must be the same,which is not possible for different gases. However,if we consider the work done per unit mass or the expansion work capacity,$W \propto n = \frac{m}{M}$. Since $m$ is constant,$W \propto \frac{1}{M}$. Comparing the molar masses: $M(NH_{3}) = 17 \ g/mol$,$M(N_{2}) = 28 \ g/mol$,$M(Cl_{2}) = 71 \ g/mol$,and $M(H_{2}S) = 34 \ g/mol$. Since $NH_{3}$ has the lowest molar mass,it will have the highest number of moles for a given mass,resulting in the maximum work done.

At the same conditions of pressure,volume,and temperature,work done is maximum for which gas if all gases have equal masses?

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