For an ideal gas,which of the following state | vedclass

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(D) $1$. For an ideal gas,the internal energy $U$ is a function of temperature only $(U = nC_vT)$. Thus,the change in internal energy $\Delta U = nC_v

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$A, B$ and $C$

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(D) $1$. For an ideal gas,the internal energy $U$ is a function of temperature only $(U = nC_vT)$. Thus,the change in internal energy $\Delta U = nC_v(T_2 - T_1)$ is valid for any process,including constant pressure. Statement $A$ is correct.$2$. In an adiabatic process,$Q = 0$. From the first law of thermodynamics,$\Delta U = Q - W$,so $\Delta U = -W$. This means the magnitude of the change in internal energy is equal to the magnitude of the work done. Statement $B$ is correct.$3$. In an isothermal process,temperature $T$ is constant. Since internal energy $U$ depends only on $T$ for an ideal gas,$\Delta U = 0$. Statement $C$ is correct.$4$. Since all statements $A, B,$ and $C$ are correct,the correct option is $D$.

For an ideal gas,which of the following statements is correct?

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