In an isobaric process of an ideal gas, the r | vedclass

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(D) In an isobaric process, the pressure remains constant.Heat exchanged is given by $Q = n C_p \Delta T$.Work done by the system is given by $W = P \

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$\frac{\gamma-1}{\gamma}$

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(D) In an isobaric process, the pressure remains constant.Heat exchanged is given by $Q = n C_p \Delta T$.Work done by the system is given by $W = P \Delta V = n R \Delta T$.Using Mayer's relation, $R = C_p - C_v$.Therefore, $W = n(C_p - C_v) \Delta T$.The ratio of work done to heat exchanged is $\frac{W}{Q} = \frac{n(C_p - C_v) \Delta T}{n C_p \Delta T} = \frac{C_p - C_v}{C_p} = 1 - \frac{C_v}{C_p}$.Since $\gamma = \frac{C_p}{C_v}$, we have $\frac{C_v}{C_p} = \frac{1}{\gamma}$.Thus, $\frac{W}{Q} = 1 - \frac{1}{\gamma} = \frac{\gamma - 1}{\gamma}$.

In an isobaric process of an ideal gas, the ratio of work done by the system $(W)$ during the expansion and the heat exchanged $(Q)$ is $(\gamma = \frac{C_p}{C_v})$

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