Since the vapor pressure of A is more than B so the mole fraction of A is more in vapor phase than liquid phase as A is more volatile hence vapor phase would be richer in A. Thus the correct option is (x_A)_liquid < (x_B)_Vapor

For an ideal solution, ΔH and Delta ΔV for mixing should be zero. P_Total = p_A + p_B and A − A, B − B and A − B interactions are nearly same.

Azeotropes are formed by the solutions which show deviations from ideal behaviour.

Acetone + ethanol is an example of solutions showing positive deviation from Raoult's law. Since acetone-ethanol attractions are weaker than acetone - acetone and ethanol-ethanol attractions.

CH₃COCH₃ + CHCl₃ is an example of solution showing negative deviation from Raoult's law since A-B attractions (acetone + chloroform) are more than A - A (acetone -acetone) and B - B( chloroform-chloroform) attractions.

Acetone + ethyl alcohol solution shows positive deviation while acetone + chloroform shows negative deviation.
Other examples:
Positive deviations - Acetone + ethyl alcohol,
acetone + benzene, water + ethyl alcohol
Negative deviations - Nitric acid + water,
benzene + chloroform

When acetone and chloroform are mixed together, hydrogen bonds are formed between them which increases intermolecular interactions hence decreases the vapour pressure showing negative deviation.

(iii) and (iv) will form ideal solutions hence do not form azeotropes. Azeotropes have same composition in liquid and vapour form when distilled.

When acetone and chloroform are mixed together, a hydrogen bond is formed between them which increases intermolecular interactions. Hence, A − B interactions are stronger than A − A and A − B interactions.

Due to stronger intermolecular interactions in acetone and chloroform lesser number of molecules vaporise resulting in low vapour pressure and high boiling point.