Asolution is made by mixing 48.0 ml of ethanol, c2h6o, and 52.0 ml of water. assuming ideal behavior, what is the vapor pressure of the solution at 20 °c?

The mass of ethanol = 0.789 g/ml (48) = 37.872 g
Number of moles of ethanol = 37.872 g/ 46g/mol = 0.8233 moles
Mass of water = 52 x 1g/ml = 52 g
Number of moles of water = 52 / 18 g/mol = 2.889 moles of water
We can calculate the mole fraction;
Mole fraction of ethanol =  0.8233/3.712 = 0.2218
Mole fraction of water  = 2.889/3.712= 0.7782
But P°(1) Vapor pressure of pure water = 17.5 torr
while P°(2) vapor pressure of pure ethanol = 43.9 torr
P(1) = 0.7782 × 17.5 = 13.6185
P(2) =0.2218 ×43.9 = 9.7370
Therefore, the P(s) = 23.3555