The specific heat at constant pressure (C_P) | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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 $1 	ext{ K}$

Vedclass · Accepted Answer

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

Vedclass · Answer

(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:

Similar Questions

When heat $Q$ is supplied to a diatomic gas of rigid molecules at constant volume,its temperature increases by $\Delta T$. The heat required to produce the same change in temperature at constant pressure is:

If a gas has $n$ degrees of freedom,the ratio of specific heats of the gas is:

Explain the difference between the expressions $C_P - C_V = R$,$C_P - C_V = \frac{R}{J}$,and $C_P - C_V = \frac{r}{J}$.

Obtain the equation for $\gamma = \frac{C_P}{C_V}$ in terms of the degree of freedom $f$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module