An amount of 700 ,J of heat is transferred to | vedclass

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(A) For an isobaric process, the heat supplied is given by $\Delta Q = n C_P \Delta T = 700 \,J$. The change in internal energy is $\Delta U = n C_V \

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$200$

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(A) For an isobaric process, the heat supplied is given by $\Delta Q = n C_P \Delta T = 700 \,J$. The change in internal energy is $\Delta U = n C_V \Delta T$. For a diatomic gas, the adiabatic index is $\gamma = \frac{C_P}{C_V} = 1.4 = \frac{7}{5}$. From the first law of thermodynamics, $\Delta Q = \Delta U + W$, so the work done by the gas is $W = \Delta Q - \Delta U$. Since $\Delta U = n C_V \Delta T = n \left(\frac{C_P}{\gamma}\right) \Delta T = \frac{\Delta Q}{\gamma}$, we have: $W = \Delta Q - \frac{\Delta Q}{\gamma} = \Delta Q \left(1 - \frac{1}{\gamma}\right)$. Substituting the values: $W = 700 \left(1 - \frac{5}{7}\right) = 700 \left(\frac{2}{7}\right) = 200 \,J$.

An amount of $700 \,J$ of heat is transferred to a diatomic gas, allowing it to expand with the pressure held constant. The work done by the gas is (in $\,J$)

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