Discussion
The ideal solution made up of 5.00 mol (mole fraction = 0.606) benzene and 3.25 mol (mole fraction = 0.394) toluene, the change in enthalpy during mixing (ΔHmix) would be :
Answer: A
ΔHmix is zero.
An ideal solution is one in which the interactions between unlike molecules (benzene-toluene) are the same as those between like molecules. Mixing then involves no net breaking or making of interactions, so no heat is absorbed or released, and ΔHmix = 0 at every composition. The whole of the negative ΔGmix in such a solution comes from the entropy of mixing, ΔGmix = −TΔSmix.
A positive ΔHmix describes a solution with positive deviations from Raoult's law, and a negative one a solution with negative deviations, so neither applies to an ideal solution, and the figure 1.0 kJ mol−1 has no basis.
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