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(C) The internal energy $(U)$ of an ideal gas is purely kinetic because there are no intermolecular forces of attraction $(U_p = 0)$. Thus,$U = U_k =

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Statement-$1$ is true,Statement-$2$ is true but Statement-$2$ is not the correct explanation of Statement-$1$.

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(C) The internal energy $(U)$ of an ideal gas is purely kinetic because there are no intermolecular forces of attraction $(U_p = 0)$. Thus,$U = U_k = \frac{3}{2} \mu R T$,which depends only on the absolute temperature $T$. Hence,Statement-$1$ is true.For a given amount of heat $\Delta Q$,the temperature change $\Delta T$ is given by $\Delta Q = \mu C \Delta T$,or $\Delta T = \frac{\Delta Q}{\mu C}$.Since the molar specific heat at constant pressure $(C_P)$ is greater than the molar specific heat at constant volume $(C_V)$,i.e.,$C_P > C_V$,it follows that for the same $\Delta Q$,$(\Delta T)_P However,Statement-$2$ describes the relationship between specific heats and temperature rise,which is not the reason why internal energy depends only on temperature. Therefore,Statement-$2$ is not the correct explanation of Statement-$1$.

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