Given below are two statements:Statement I: F | vedclass

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(D) Statement $I$ is false because for an ideal gas,the heat capacity at constant pressure $(C_p)$ is always greater than the heat capacity at constan

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Statement $I$ is false but Statement $II$ is true

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(D) Statement $I$ is false because for an ideal gas,the heat capacity at constant pressure $(C_p)$ is always greater than the heat capacity at constant volume $(C_v)$,as defined by the relation $C_p - C_v = R$.Statement $II$ is true because in a constant volume process (isochoric process),the change in volume $\Delta V = 0$. Since work done $W = P\Delta V$,it follows that $W = 0$. According to the first law of thermodynamics,$\Delta U = Q + W$. Since $W = 0$,the heat added $(Q_v)$ is entirely used to increase the internal energy $(\Delta U)$,which corresponds to an increase in the chaotic motion of molecules and is reflected as a rise in temperature.

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