The combination of plots which do not represe | vedclass

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(A) For an ideal gas undergoing isothermal expansion,the temperature $T$ is constant. $(a)$ According to Boyle's Law,$P = nRT / V_m$. Thus,$P$ vs $1/V

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$b$ and $d$

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(A) For an ideal gas undergoing isothermal expansion,the temperature $T$ is constant. $(a)$ According to Boyle's Law,$P = nRT / V_m$. Thus,$P$ vs $1/V_m$ is a straight line passing through the origin. This represents isothermal expansion. $(b)$ $P$ vs $V_m$ should be a rectangular hyperbola $(P \propto 1/V_m)$,not a straight line. This plot is incorrect. $(c)$ For an ideal gas,$PV_m = RT$. Since $T$ is constant,$PV_m$ is constant regardless of $P$. This plot is correct. $(d)$ For an ideal gas,internal energy $U$ depends only on temperature $(U = f(T))$. Since the process is isothermal,$U$ must be constant. The plot shows $U$ increasing with $V_m$,which is incorrect. Therefore,plots $(b)$ and $(d)$ do not represent isothermal expansion.

The combination of plots which do not represent isothermal expansion of an ideal gas is

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