For two pure volatile liquids X and Y , attractive intermolecular interactions of both X - X and Y - Y are weaker than those of X - Y . The total vapour pressure of an equimolar solution of X and Y is p_ total . The vapour pressure of pure X and pure Y are p^0_X and p^0_Y , respectively. Which one of the following relations is correct?

Step-by-step solution

Given that the attractive intermolecular interactions of X-Y are stronger than those of X-X and Y-Y. This implies that the molecules of X and Y are held more tightly in the solution than in their pure liquid states, decreasing their escaping tendency into the vapour phase. Consequently, the solution exhibits a negative deviation from Raoult's law. For an ideal solution, the total vapour pressure is given by: p_ ideal = x_X p^0_X + x_Y p^0_Y For an equimolar solution, x_X = x_Y = 1 2 . p_ ideal = p^0_X + p^0_Y 2 Sin