Question

Question 40 (8 points) What is the vapor pressure at 35°C of a solution made by dissolving 44.6.g of sucrose, C12H22011, in 62.3 g of water? The vapor pressure of pure water at 35°C is 42.2 torr.

please show work?

Answer 1

at Answers Given, mass of sucrose dissolved = nu.6g mass of water 62.3g vapour pressure of puse water at 3500 35°C(PO)= 42.2 Now, we have to calculate vapons pressure of solution af tes dissowing sucione 35°C 2. Р Now, from Raolalte Law of vapous pressure. Psolution = X Solvent po where Psolution = vapous pressure of solution X solvent mole fraction of solvent po = vapour pressure of water (pluse) moles of H₂O nows, Mole fraction of Solvent total moles of particle WH₂O fusthes, moles of H₂O MH₂O 62.3 3.46 WC 12 M2 2011 moles of sucrose = MC12 M2 2011 44.6 0.130 342:3 total moles of particle = moles of H₂O + moles of C 12 H2 2011 3.46 + 0.130 3.59

So, mole Fraction of Solvent moles of 120 total motes of particle X Solvent 3.46 3.59 X Solvent = 0.9637 Therefore, vapous pressure of Solution Psolution X Solvent po 0.9637 x 42.2 toss Psolution 40.66 toss was