At 28.0°C, the vapor pressure of pure carbon disulfide, CS₂, is 378.7 torr, while that of acetone, C₃H₆O, is 228.9 torr. What is the vapor pressure, at 28.0°C, of a solution made by mixing 0.250 moles of carbon disulfide and 0.450 moles of acetone, if Raoult's Law is obeyed?Hint: Organizing the given information into moles and mole fraction of each component will help in solving this problem.

Question

Quizplus · Accepted Answer

The vapor pressure of the solution is calculated using Raoult's Law: P_solution = (X_CS2 * P_pure_CS2) + (X_acetone * P_pure_acetone). The mole fraction of CS2 (X_CS2) is 0.250 / (0.250 + 0.450) = 0.357, and the mole fraction of acetone (X_acetone) is 0.450 / (0.250 + 0.450) = 0.643. Therefore, P_solution = (0.357 * 378.7) + (0.643 * 228.9) = 282 torr.

At 280°C, the Vapor Pressure of Pure Carbon Disulfide, CS2, Is

At 280°C, the Vapor Pressure of Pure Carbon Disulfide, CS₂, Is