1. The problem statement, all variables and given/known data How much water would be needed to completely dissolve 1.48L of the gas at a pressure of 730torrand a temperature of 28∘C? A gas has a Henry's law constant of 0.190M/atm 2. Relevant equations S=kH * Pgas 3. The attempt at a solution 730 torr= .960526316 atm S=(.190M/atm)(.960526316 atm) S= .1825 M .1825 mol = X = .2701 moles 1 L 1.48L After solving that part I don't understand how to get liters of water. Maybe PV=nRT... but I tried that and I got the answer wrong.