The specific heat at constant pressure (C_P) | vedclass

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(A) By definition,specific heat at constant volume $(C_V)$ is the heat required to raise the temperature of $1 	ext{ mole}$ of a gas by $1 	ext{ K}$

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At constant pressure,work is done in expanding the gas.

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(A) By definition,specific heat at constant volume $(C_V)$ is the heat required to raise the temperature of $1 	ext{ mole}$ of a gas by $1 	ext{ K}$ while keeping the volume constant. In this case,no external work is done $(W = 0)$,so all the heat supplied is used to increase the internal energy of the gas.However,at constant pressure $(C_P)$,when heat is supplied to the gas,it not only increases the internal energy but also performs external work $(W = P \Delta V)$ to expand the gas against the constant external pressure.According to the first law of thermodynamics,$\Delta Q = \Delta U + W$. Since $C_P$ requires additional energy to perform this expansion work,more heat must be supplied to achieve the same temperature rise compared to the constant volume process. Therefore,$C_P > C_V$.

The specific heat at constant pressure $(C_P)$ is greater than the specific heat at constant volume $(C_V)$ for the same gas because:

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