Which of the following is correct for a solution showing positive deviations from Raoult’s law?

ΔV = +ve, ΔH = +ve

For a solution showing positive deviations from Raoult's law, the correct option is:

(1) $\Delta V = +\text{ve}$, $\Delta H = +\text{ve}$.

Positive deviations from Raoult's law occur when the intermolecular forces between the components of the solution are stronger than expected based on ideal behavior. This can happen when there are significant intermolecular interactions or bonding between the solute and solvent molecules.

In such cases, the enthalpy of mixing ($\Delta H$) is positive because energy is required to break the stronger intermolecular forces in order to mix the components. The positive $\Delta H$ value indicates an endothermic process.

Additionally, the change in volume ($\Delta V$) of the solution upon mixing is positive. This indicates an increase in volume compared to what would be expected based on ideal behavior. Positive $\Delta V$ suggests that the molecules of the components occupy more space when mixed together, possibly due to changes in solvation or molecular interactions.

Therefore, the correct option is (1) $\Delta V = +\text{ve}$, $\Delta H = +\text{ve}$ for a solution showing positive deviations from Raoult's law.