An ideal gas is expanded from (p_1, V_1, T_1) | vedclass

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(B) Statement $A$: For irreversible compression,$W = -p_{ext} \Delta V$. Compressing against the maximum possible external pressure $(p_1)$ results in

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$A, B, D$

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(B) Statement $A$: For irreversible compression,$W = -p_{ext} \Delta V$. Compressing against the maximum possible external pressure $(p_1)$ results in the maximum work done on the gas.Statement $B$: For an ideal gas,the $p-V$ curve for an adiabatic process is steeper than that for an isothermal process. Thus,the area under the curve (work done) for reversible expansion from $V_1$ to $V_2$ is smaller for the adiabatic process.Statement $C$: For an ideal gas,$\Delta U = nC_v \Delta T$. If $T_1 = T_2$,$\Delta U = 0$. For adiabatic expansion,$T$ decreases,so $\Delta T Statement $D$: Free expansion occurs against $p_{ext} = 0$,so $W = 0$. For an ideal gas,$\Delta U = q + W = 0$,implying $\Delta T = 0$ (isothermal). Since $q = 0$,it is also adiabatic. Thus,$D$ is correct.Therefore,the correct statements are $A, B, D$.

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