Calculate the vapor pressure at 25 °C of a solution containing 99.5 g sucrose (C₁₂H₂₂O₁₁) and 300.0 mL water.

The vapor pressure of pure water at 25 °C is 23.8 torr. Assume the density of water is 1.00 g/mL.

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SORT You are given the mass of sucrose and volume of water in a solution. You are also given the vapor pressure and density of pure water and asked to find the vapor pressure of the solution. STRATEGIZE Raoult's law relates the vapor pressure of a solution to the mole fraction of the solvent and the vapor pressure of the pure solvent. Begin by calculating the amount in moles of sucrose and water. Calculate the mole fraction of the solvent from the calculated amounts of solute and solvent. Then use Raoult's law to calculate the vapor pressure of the solution. GIVEN: 99.5 g C12H22O11 300.0 mL H₂O PH₂O dH₂0 FIND: Psolution CONCEPTUAL PLAN g C12H22011 mL H₂O = 23.8 torr at 25 °C 1.00 g/mL mol C12H22011 1 mol C₁2H₂2011 342.30 g C12H22011 1.00 g 1 mL g H₂O mol C12H22011, mol H₂O XH₂0 XH,O, PH,o 1 mol H₂O 18.02 g H₂O mol H₂O XH₂O PHO *Hạo+nC_zHzzO11 P solution Psolution = XH₂OPH₂0