A solution is made by mixing 33.0 ml of ethanol, C2H6O and 67.0 ml of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 degree C? Ethanol =.789 g/ml 43.9 torr. water =.998 g/ml 17.5 torr

Question

Thaddeus Vaughn

Chemistry

26 June, 23:37

A solution is made by mixing 33.0 ml of ethanol, C2H6O and 67.0 ml of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 degree C? Ethanol =.789 g/ml 43.9 torr. water =.998 g/ml 17.5 torr

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Mauricio Morse · Answer 1

Grams ethanol = 33 ml times. 789 gms/ml = 26.037 gms

Moles ethanol = 26.037 gms / 46 gms/mole =.57 moles

Moles water = 67 ml or 67 grams/18 gms/mole = 3.22 moles

total moles =.57 + 3.72 = 4.29 moles

Mole fraction ethanol =.57 moles ethanol / 4.29 moles total = 0.13

Moles fraction water = 3.72 moles water / 4.29 moles total = 0.87

Partial pressure of ethanol = mole fraction ethanol (.13) _ times VP ethanol 43.9 torr) = 5.707 torr

partial pressure water = mole fraction water. 87) times VP water (l7.5 torr) = 15.23 torr

Total vapor pressure over solution = 5.71 torr + 15.23 torr = 20.94 torr