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(A) For an ideal gas:$1$. Internal energy $U$ and enthalpy $H$ are functions of temperature only,i.e.,$U = f(T)$ and $H = f(T)$. Thus,statement $(a)$

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$(a), (c)$ and $(d)$

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(A) For an ideal gas:$1$. Internal energy $U$ and enthalpy $H$ are functions of temperature only,i.e.,$U = f(T)$ and $H = f(T)$. Thus,statement $(a)$ is true.$2$. The compressibility factor $Z$ for an ideal gas is defined as $Z = \frac{PV}{nRT} = 1$. Thus,statement $(b)$ is false.$3$. For an ideal gas,the molar heat capacity relation is $C_{P,m} - C_{V,m} = R$. Thus,statement $(c)$ is true.$4$. The relation $dU = C_V dT$ holds for an ideal gas for any process,whether reversible or irreversible. Thus,statement $(d)$ is true.Therefore,statements $(a), (c),$ and $(d)$ are correct.

For one mole of an ideal gas,which of these statements must be true?
$(a)$ $U$ and $H$ each depend only on temperature.
$(b)$ Compressibility factor $Z$ is not equal to $1$.
$(c)$ $C_{P,m} - C_{V,m} = R$
$(d)$ $dU = C_V dT$ for any process.

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For one mole of an ideal gas,which of these statements must be true?$(a)$ $U$ and $H$ each depend only on temperature.$(b)$ Compressibility factor $Z$ is not equal to $1$.$(c)$ $C_{P,m} - C_{V,m} = R$$(d)$ $dU = C_V dT$ for any process.