Problem: Calculate the vapor pressure (in torr) at 310 K in a solution prepared by dissolving 12.3 g of the non-volatile non-electrolye sucrose (342.3 g/mol) in 141 g of water. The vapor pressure of water at 310 K is 47.08 torr.  Enter your answer to 2 decimal places.A. 0.06 torrB. 64.86 torrC. 0.215 torrD. 46.86 torrE. 17.72 torr

We’re being asked to calculate the vapor pressure (in torr) of a solution in a solution prepared by dissolving 12.3 g of the non-volatile non-electrolye sucrose (342.3 g/mol) in 141 g of water.

The vapor pressure of a solution can be given by Raoult’s Law:

$\boxed{{\mathbf{P}}_{\mathbf{solution}}\mathbf{=}\mathbf{P}{\mathbf{°}}_{\mathbf{solvent}}{\mathbf{\chi }}_{\mathbf{solvent}}}$

where P˚ = vapor pressure of solvent and χ = mole fraction of solvent. 

We're going to calculate the vapor pressure of the solution using the following steps:

Step 1: Calculate the moles of solvent (water) and moles of solute (sucrose)
Step 2: Calculate the mole fraction of solvent (water)
Step 3: Calculate the vapor pressure of the solution

Mole fraction is given by: