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**:

$\overline{){{\mathbf{P}}}_{{\mathbf{solution}}}{\mathbf{=}}{\mathbf{P}}{{\mathbf{\xb0}}}_{{\mathbf{solvent}}}{{\mathbf{\chi}}}_{{\mathbf{solvent}}}}$

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:

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 torr

B. 64.86 torr

C. 0.215 torr

D. 46.86 torr

E. 17.72 torr