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Feb 25th, 2015

The calculation of vapor pressure for a solution uses Raoult's law: PA = XA PA°

PA = vapor pressure of the solution

XA = mole fraction of the solvent
(a common error is to use the mole fraction of solute)

PA° = vapor pressure of the pure solvent

Thus, as the amount of solute increases, the mole fraction of the solvent decreases as does the vapor pressure of the solution.

First, moles of both substances need to be calculated.

moles = mass / molecular weight

moles of pure H2O = 180.16 g / 18 g/mol = 10.01 moles

moles of C6H12O6= 18.016 g / ((6x12)+ (12x1) + (16x6)) g/mol = 18.016 g/ (72+12+96) g/mol = 18.016 g / 180 g/mol = 0.1 moles

Now, you need to sum moles: 10.01 moles + 0.1 moles = 10.11 moles

X(water) = 10.01 moles / 10.11 moles = 0.990

P (water) = 0.990 x 23.76 mmHg = 23.52 mm Hg

The final answer is d. 23.52 mm Hg

Feb 26th, 2015

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Feb 25th, 2015
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Feb 25th, 2015
Dec 9th, 2016
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