When an ideal diatomic gas is heated at const | vedclass

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(D) When a gas is heated at constant pressure,the heat supplied $(\Delta Q)_p$ is used to increase the internal energy $(\Delta U)$ and to perform wor

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$5/7$

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(D) When a gas is heated at constant pressure,the heat supplied $(\Delta Q)_p$ is used to increase the internal energy $(\Delta U)$ and to perform work $(\Delta W)$ against external pressure.$(\Delta Q)_p = \Delta U + \Delta W$Using the molar heat capacities,we have $\mu C_p \Delta T = \mu C_v \Delta T + P \Delta V$.The fraction of heat energy used to increase the internal energy is given by the ratio $\frac{\Delta U}{(\Delta Q)_p} = \frac{\mu C_v \Delta T}{\mu C_p \Delta T} = \frac{C_v}{C_p} = \frac{1}{\gamma}$.For a diatomic gas,the adiabatic index is $\gamma = 7/5$.Therefore,the fraction is $\frac{1}{7/5} = 5/7$.

When an ideal diatomic gas is heated at constant pressure,the fraction of the heat energy supplied which increases the internal energy of the gas is:

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