A solution is made by mixing 45.0 mL of ethanol, C2H6O, and 55.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C?
Constants @ 20*C:
ethanol = 0.789(Density) & 43.9(Vapor Pressure - Torr)
water = 0.998(Density) & 17.5(Vapor Pressure - Torr)
P = PaXa + PbXb
mass of ethanol = 45 x 0.789= 35.5 gm = 35.5/46 = 0.772 moles,
mass of water = 0.998 x 55 = 54.89 gm = 54.89/18 = 3.05 moles ,
Xa = (0.772)/(0.772+3.05) = 0.202 , Xb = 1-0.202 = 0.798,
P = (0.202)(43.9) + (0.798)(17.5) = 22.83 Torr
A solution is made by mixing 45.0 mL of ethanol, C2H6O, and 55.0 mL of water. Assuming ideal behavior, what is the va...
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