The difference between C_p and C_v can be der | vedclass

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(A) For an ideal gas,the enthalpy is defined as $H = U + PV$. Since $PV = nRT$ for $n$ moles of an ideal gas,we have $H = U + nRT$. Differentiating wi

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$10R$

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(A) For an ideal gas,the enthalpy is defined as $H = U + PV$. Since $PV = nRT$ for $n$ moles of an ideal gas,we have $H = U + nRT$. Differentiating with respect to temperature $T$ at constant pressure,we get $\frac{dH}{dT} = \frac{dU}{dT} + nR$. By definition,$C_p = \frac{dH}{dT}$ and $C_v = \frac{dU}{dT}$. Therefore,$C_p - C_v = nR$. Given $n = 10$,the difference is $10R$.

The difference between $C_p$ and $C_v$ can be derived using the empirical relation $H = U + PV$. Calculate the difference between $C_p$ and $C_v$ for $10$ moles of an ideal gas.

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