According to my textbook, the change in internal energy for all isothermal processes in a perfect gas is equal to zero. However, in a problem I did, for a reversible isothermal condensation (from H2O(g) to H2O(l)), I was given the change in enthalpy (delta H) and therefore according to the formula delta H = delta U + deltaNRT, there would be a change in internal energy (since we have the enthalpy and there's a change in moles of gas). Isn't this contradictory? Any help explaining this to me would be appreciated
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Topic: internal energy (Read 2432 times)