122ch13d_001

122ch13d_001 - 37 13.50) 38 13.55 39 13.58) 13.59)...

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39 13.58) 13.59) Calculate the VP of H 2 O for various aqueous solutions of nonvolatile solutes. Given the masses of solute and solvent we can find moles and then mole fractions. Then use Raoult’s Law, which gives the VP of a volatile substance above a solution (in this case only the H 2 O since the solute is nonvolatile): P H 2 O = X H 2 O P ° H 2 O P H 2 O / VP of H 2 O (solvent) above soln P ° H 2 O / VP of pure H 2 O (solvent) X H 2 O / mole fraction of H 2 O (solvent) * continued on next page *
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40 13.59) (cont.) Could find ) P H 2 O first ( ) P H 2 O = X solute P ° H 2 O ) and then find P H 2 O ) P H 2 O = P ° H 2 O P H 2 O ˆ P H 2 O = P ° H 2 O ) P H 2 O - longer and messier (do it the way I have it below) a) P ° H 2 O = 187.5 torr at 338 K (65°C) 1 mol C 12 H 22 O 11 ? mol C 12 H 22 O 11 = 22.5 g C 12 H 22 O 11 x ----------------------- = 0.065 7 3 mol C 12 H 22 O 11 342.3 g C 12 H 22 O 11 1 mol H 2 O ? mol H 2 O = 200.0 g H 2 O x ------------------
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This note was uploaded on 07/17/2008 for the course CHEM 122 taught by Professor Zellmer during the Summer '07 term at Ohio State.

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122ch13d_001 - 37 13.50) 38 13.55 39 13.58) 13.59)...

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