Need help with chem 2. Hopefully someone has an idea... Calculate the vapor pressure (in torr) at 310 K in a solution prepared by dissolving 23.8 g of the non-volatile non-electrolyte sucrose in 126 g of water. The vapor pressure of water at 310 K is 47.08 torr. Thanks.
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P = X solvent * P solvent X solvent = moles of solvent/total moles Molar mass of water = 18 g/mol Moles of solvent (water) = 126/18 = 7 moles Molar mass of sucrose = 342.3 g/mol Moles of solute (sucrose) = 23.8g/342.3 = .06953 Total moles = 7.06953 moles X solvent = moles of water/total moles = 7 mol/7.06952 mol = .990166 P = X solvent * P solvent = .990166 * (47.08 torr) = 46.617 ~ 46.6 torr (3 sig figs) Hope that's right. Just had a test over it along with other stuff.
Well, if you use moles of sucrose, you can subtract its torr from the water torr and still get the answer.
