If 0.600 mol of a nonvolatile nonelectrolyte are dissolved in 3.70 mol of water, what is the vapor pressure ph2o of the resulting solution? the vapor pressure of pure water is 23.8 torr at 25 ? c .

To get the vapor pressure of the resulting solution, we use the Raoult’s Law:

Psolution = (χsolvent) (P°solvent)

1st: Calculate the mol fraction of the solvent. In this case, water is the solvent.

χsolvent = 3.7 mol / (3.7 mol + 0.6 mol)

χsolvent = 0.86

2nd: Calculate the vapor pressure.

Psolution = (0.86) (23.8 torr)

Psolution = 20.48 torr

1= 26.17

2= 1.17

3=30.86

4=5.86

just took the assigment on edge

okay i have so many questions. but the big one here is: um wt..f is this mess? ?