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(C) The ideal gas equation is given by $pV = nRT = \frac{m}{M}RT$,where $m$ is the mass of the gas and $M$ is the molar mass.For a fixed temperature $

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$m_1 < m_2$

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(C) The ideal gas equation is given by $pV = nRT = \frac{m}{M}RT$,where $m$ is the mass of the gas and $M$ is the molar mass.For a fixed temperature $T$,we have $pV = 	ext{constant} 	imes m$,which implies $m = \frac{pVM}{RT}$.For a constant pressure $p$,we can see from the graph that for the same pressure,the volume $V_2$ corresponding to mass $m_2$ is greater than the volume $V_1$ corresponding to mass $m_1$ (i.e.,$V_2 > V_1$).Since $m = \frac{pVM}{RT}$,for a constant $p, T,$ and $M$,we have $m \propto V$.Since $V_2 > V_1$,it follows that $m_2 > m_1$ or $m_1 < m_2$.

Two different isotherms representing the relationship between pressure $p$ and volume $V$ at a given temperature for the same ideal gas are shown for masses $m_1$ and $m_2$ of the gas respectively in the figure given. Then:

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