1. The problem statement, all variables and given/known data 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? 2. Relevant equations VP of solution = mole fraction of solvent * VP of pure solvent 3. 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.