Two volatile liquids, A and B, form a perfectly ideal solution. If of A and of B are mixed at constant temperature and pressure, the theoretical entropy of mixing () is strictly positive. For this exa

Question

Two volatile liquids, A and B, form a perfectly ideal solution. If $0.5	ext{ moles}$ of A and $0.5	ext{ moles}$ of B are mixed at constant temperature and pressure, the theoretical entropy of mixing ($\Delta S_{mix}$) is strictly positive. For this exact ideal mixing process, what is the exact magnitude of the overall enthalpy of mixing ($\Delta H_{mix}$) in Joules?

Prashant Kotian · Accepted Answer

Correct answer: 0. By standard thermodynamic definition, an ideal solution features intermolecular forces (A-B) that are exactly identical to the pure state forces (A-A and B-B). Because breaking the old interactions costs the exact same amount of energy as is released upon forming the new interactions, the net enthalpy change () is strictly .

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