When an ideal diatomic gas is heated at const | vedclass

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(D) For an ideal diatomic gas,the molar heat capacity at constant pressure is $C_p = \frac{7}{2}R$ and the molar heat capacity at constant volume is $

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$5/7$

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(D) For an ideal diatomic gas,the molar heat capacity at constant pressure is $C_p = \frac{7}{2}R$ and the molar heat capacity at constant volume is $C_v = \frac{5}{2}R$.When heat $dQ$ is supplied at constant pressure,the total heat supplied is $dQ = n C_p dT = n (\frac{7}{2}R) dT$.The heat utilized to increase the internal energy is $dU = n C_v dT = n (\frac{5}{2}R) dT$.The fraction of heat utilized to increase internal energy is $f = \frac{dU}{dQ} = \frac{n (\frac{5}{2}R) dT}{n (\frac{7}{2}R) dT} = \frac{5/2}{7/2} = \frac{5}{7}$.

When an ideal diatomic gas is heated at constant pressure,the fraction of the heat utilized to increase the internal energy of the gas is

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