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When 1 mol of a gas is heated at constant volume, temperature is raised from 298 to 308 K. If heat supplied to the gas is 500 J, then which statement is correct?

1. q = w = 500 J, ΔU = 0
2. ΔU = 500 J, w = 0
3. q = w = 500 J, ΔU = 500 J
4. ΔU = 0, q = w = -500 J

Correct answer: ΔU = 500 J, w = 0

Solution

At constant volume, no work is done (w = 0). The heat supplied (q) is entirely used to increase the internal energy (ΔU). Thus, ΔU = q = 500 J.

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