Answer:
The vapor pressure of the solution is 284.29 mmHg
Explanation:
From Raoult's law
Vapor pressure of solution = mole fraction of solvent × vapor pressure of solvent
Mass of solute (acetone) = 30.5 g
MW of acetone (CH3COCH3) = 58 g/mol
Number of moles of solute = mass/MW = 30.5/58 = 0.526 mol
Mass of solvent (ethyl acetate) = 23.5g
MW of ethyl acetate (CH3COOC2H5) = 88 g/mol
Number of moles of solvent = mass/MW = 23.5/88 = 0.267 mol
Volume of solvent = 0.267×22.4×1000 = 5980.8 cm^3
Vapor pressure of solvent (P) = nRT/V
n is number of moles of solvent = 0.267 mol
R is gas constant = 82.057 cm^3.atm/mol.K
T is temperature of solution = 30°C = 30+273 = 303 K
V is volume of the solvent = 5980.8 cm^3
P = 0.267×82.057×303/5980.8 = 1.11 atm = 1.11×760 = 843.6 mmHg
Total moles of solution = moles of solute + moles of solvent = 0.526 + 0.267 = 0.793 mol
Mole fraction of solvent = moles of solvent/moles of solution = 0.267/0.793 = 0.337
Vapor pressure of solution = 0.337 × 843.6 mmHg = 284.29 mmHg