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(B) For an ideal gas,the molar heat capacity at constant pressure is given by $C_P = C_V + R = \frac{f}{2}R + R = (1 + \frac{f}{2})R$.Given the degree

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$100$

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(B) For an ideal gas,the molar heat capacity at constant pressure is given by $C_P = C_V + R = \frac{f}{2}R + R = (1 + \frac{f}{2})R$.Given the degree of freedom $f = 6$,we have $C_P = (1 + \frac{6}{2})R = 4R$.For a process at constant pressure,the work done is $W = nR\Delta T = 25 \ J$.The heat absorbed by the gas is $Q = nC_P\Delta T$.Substituting $C_P = 4R$,we get $Q = n(4R)\Delta T = 4(nR\Delta T)$.Since $nR\Delta T = W = 25 \ J$,the heat absorbed is $Q = 4 	imes 25 \ J = 100 \ J$.

The average degree of freedom per molecule of a gas is $6$. The gas performs $25 \ J$ of work while expanding at constant pressure. The heat absorbed by the gas is .... $J$

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