"a solution is made by mixing 44.0 ml of ethanol, c2h6o, and 56.0 ml of water. assuming ideal behavior, what is the vapor pressure of the solution at 20 °c

Vapor pressure of the solution = Partial pressure of ethanol + partial pressure of water.

Partial pressure of ethanol can be calculated from the molefraction of ethanol and vapor pressure of pure ethanol at

Density of ethanol = 0.800 g/mL

Finding out mass of ethanol =

Moles of ethanol =

Density of water = 1.00 g/mL

Mass of water =

Moles of water =

Total number of moles of the solution = 0.764 mol + 3.11 mol = 3.874 mol

Molefraction of ethanol =

Molefraction of water =

Vapor pressure of pure ethanol at

Vapor pressure of pure water at

Using Raoult's law to find out partial pressures:

= 11.68 mmHg

= 14.05 mmHg

Total vapor pressure of the solution = 11.68 mmHg + 14.05 mmHg

= 25.73 mmHg

1 is the answer to this problem