Question:
A diatomic gas with rigid molecules does \(10\ \mathrm{J}\) of work when expanded at constant pressure. What would be the heat energy absorbed by the gas, in this process ?
A diatomic gas with rigid molecules does \(10\ \mathrm{J}\) of work when expanded at constant pressure. What would be the heat energy absorbed by the gas, in this process ?
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For a rigid diatomic gas \(C_p = \frac{7}{2}R\) and the work at constant pressure is \(nR\Delta T\); so \(Q = \frac{7}{2}W\).
Updated On: Nov 11, 2026
- \(35\ \mathrm{J}\)
- \(30\ \mathrm{J}\)
- \(25\ \mathrm{J}\)
- \(40\ \mathrm{J}\)
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The Correct Option is A
Solution and Explanation
At constant pressure: \(W = P\Delta V = nR\Delta T = 10\ \mathrm{J}\).
A rigid diatomic molecule has 5 degrees of freedom, so \(C_p = \frac{7}{2}R\).
Heat absorbed: \(Q = nC_p\Delta T = \frac{7}{2}nR\Delta T = \frac{7}{2}\times10 = 35\ \mathrm{J}\).
Answer: (1) \(35\ \mathrm{J}\)
A rigid diatomic molecule has 5 degrees of freedom, so \(C_p = \frac{7}{2}R\).
Heat absorbed: \(Q = nC_p\Delta T = \frac{7}{2}nR\Delta T = \frac{7}{2}\times10 = 35\ \mathrm{J}\).
Answer: (1) \(35\ \mathrm{J}\)
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