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(A) The first law of thermodynamics is given by $\Delta E = q + w$. $(A)$ For an isochoric process,$\Delta V = 0$,so the work done $w = -P_{ext} \Delt

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For an isochoric process,$\Delta E = q$

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(A) The first law of thermodynamics is given by $\Delta E = q + w$. $(A)$ For an isochoric process,$\Delta V = 0$,so the work done $w = -P_{ext} \Delta V = 0$. Therefore,$\Delta E = q$. $(B)$ For an adiabatic process,$q = 0$,so $\Delta E = w$. $(C)$ For an isothermal process,$\Delta T = 0$,which implies $\Delta E = 0$ for an ideal gas,so $q = -w$. $(D)$ For a cyclic process,the change in state function $\Delta E = 0$,therefore $q = -w$.

Based on the first law of thermodynamics,which one of the following is correct?

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