A solution is made by mixing 36.0 mL of ethanol, C2H6O, and 64.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20
Vap pressure of ethanol at 20 degc is 59.3 mm Hg Vap pressure of water at 20 degc is 17.5 mm Hg Mol wt of ethanol is 46.07 g/mol Mol wt of water is 18 Density of etanol is 0.789 gm / cc Densiity of water 1 gm / cc Given soln contains Moles of ethanol is 36*0.789/46.07 which is 0.62 Moles of water is 64/18 which is 3.55 moles Total moles in given soln 4.17 Mole fraction of ethanol = 0.62/4.17 which is 0.1486 Mole fraction of water = 3.55/4.17 which is 0.8514 By Raoult's law Partial pressure of ethanol = 59.3*0.1486 which is 8.81 mm Hg Partial pressure of water = 17.5*0.8514 which is 14.9 mm Hg Therefore vap pressure of soln which is the sum of partial pressure of ethanol + and partial pressure of water stands at 8.81+14.9 = 23.71 mm Hg
Get Answers For Free
Most questions answered within 1 hours.