The vapor pressure of pure water at 45 degrees C is 71.9 mm Hg. What is the vapor pressure when 18g of sucrose (MM = 342.3g/mol) is added to 82g of water?
VP of solution = mole fraction of solvent * VP of pure solvent
The Attempt at a Solution
82g of water / (18g/mol) = 4.555... moles of water.
18g of sucrose / (342.3g/mol) = 0.0525 moles of water
Mole fraction of solvent (water) = 0.988.
0.988 * 71.9 mm Hg = new vapor pressure of 71.1 mm Hg.
Is my work correct? It's 3 AM here and I'm just a bit concerned about how accurate I am in doing these practice problems.