Question

When 1 mole of A is mixed with 1 mole of B, the temperature of the solution increases. Is it an ideal solution? If not, why?

Answer 1

No, it is not an ideal solution because the temperature of the solution increases when 1 mole of A is mixed with 1 mole of B. This indicates that the mixing process is exothermic, meaning heat is released.

In an ideal solution, the enthalpy of mixing `Delta H_"mixing"` is zero, and there is no temperature change upon mixing because the intermolecular forces between A-A, B-B, and A-B are all similar.

Since the temperature increases, `Delta H_"mixing"` < 0, which is a characteristic of a non-ideal solution showing negative deviation from Raoult’s law due to stronger A-B interactions compared to A-A and B-B.