The correct option is (d) 398.246 mm Hg
For explanation: Given,
Mass of solute, m2 = 1.5 grams
Molar mass of solute, M2 = 100
Vapor pressure of pure CS2, p^01 = 400 mm Hg
Volume of solvent, ρ = 200 ml
Density of solvent, ρ = 1.3 g/cc
Number of moles of solute, n2 = m2/MW = 1.5/100 = 0.015 mole
From the law of relative lowering of vapor pressure, Δp1 = p^01X2, where X2 is the mole fraction of solute and Δp1 is the difference in pressure.
Mass of solvent, m1 = ρ x V = 1.3 x 200 = 260 grams
Number of moles of solvent, n2 = 260g/[(12 + 32 + 32)g/mole] = 3.421
Since the solution is dilute we can approximate X2 = n2/(n1 + n2) ≈ n2/n1 (since n2<< n1)
Using ∆p1 = p^01X2,
∆p1 = (400 mg of Hg) (0.015/3.421) = 1.754 mm of Hg
Using Δp1 = p^01 – p1, we get p1 = p^01 – Δp1
Hence, resulting lowered vapor pressure, p1 = 400 mm Hg – 1.754 mm Hg = 398.246 mm Hg.