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The internal energy is dependent on temperature and an isothermal reaction takes place at constant temperature. Thus, in any isothermal process involving only ideal gases, delta U=0. This is because the energy gained as heat (q) is equal to the amount of work done by the system (q = -w).
Anisha Chandra 1K wrote:Is the delta U of an isothermal irreversible reaction also equal to 0, like it is for an isothermal reversible reaction? If it's not equal to 0, why is that?
I'm having trouble wrapping my head around an isothermal irreversible expansion. In isothermal reversible expansions, all the energy transferred to the surroundings by the work of expansion is immediately replace by heat flowing in from the surroundings to the system, keeping the temperature between surroundings and system any equilibrium. In order for this to happen, the expansion must happen slowly and reversibly. How would an isothermal irreversible expansion take place?
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