The expansion of an ideal gas of mass m at a | vedclass

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(C) From the ideal gas equation,$PV = nRT$,where $n = \frac{m}{M}$ ($M$ is the molar mass).Thus,$V = \frac{mR}{MP} T$.In the given graph,the $V-T$ plo

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$B$

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(C) From the ideal gas equation,$PV = nRT$,where $n = \frac{m}{M}$ ($M$ is the molar mass).Thus,$V = \frac{mR}{MP} T$.In the given graph,the $V-T$ plot is a straight line passing through absolute zero $(-273.15\, ^\circ	ext{C})$,where the slope is $S = \frac{mR}{MP}$.For the first case,the slope is $S_1 = \frac{mR}{MP}$.For the second case,the mass is $2m$ and the pressure is $2P$,so the new slope is $S_2 = \frac{(2m)R}{M(2P)} = \frac{mR}{MP}$.Since $S_1 = S_2$,the slope remains unchanged.Therefore,the expansion is given by the same straight line $B$.

The expansion of an ideal gas of mass $m$ at a constant pressure $P$ is given by the straight line $B$. Then the expansion of the same ideal gas of mass $2\, m$ at a pressure $2\,P$ is given by the straight line

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