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(C) For an ideal gas,the heat supplied at constant pressure is given by $\Delta Q = n C_p \Delta T$.The change in internal energy is given by $\Delta

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$2: 5: 7$

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(C) For an ideal gas,the heat supplied at constant pressure is given by $\Delta Q = n C_p \Delta T$.The change in internal energy is given by $\Delta U = n C_v \Delta T$.The work done at constant pressure is $\Delta W = P \Delta V = n R \Delta T$.Therefore,the ratio is $\Delta W : \Delta U : \Delta Q = n R \Delta T : n C_v \Delta T : n C_p \Delta T = R : C_v : C_p$.For a diatomic gas,the degrees of freedom $f = 5$.Thus,$C_v = \frac{f}{2} R = \frac{5}{2} R$.Using Mayer's relation,$C_p = C_v + R = \frac{5}{2} R + R = \frac{7}{2} R$.Substituting these values into the ratio: $R : \frac{5}{2} R : \frac{7}{2} R = 1 : \frac{5}{2} : \frac{7}{2}$.Multiplying by $2$,we get the ratio $2 : 5 : 7$.

If $\Delta Q$ is the amount of heat supplied to $n$ moles of a diatomic gas at constant pressure,$\Delta U$ is the change in internal energy,and $\Delta W$ is the work done,then the ratio $\Delta W : \Delta U : \Delta Q$ is

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