Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g ethanol (M = 46 g/mol) in 500 mL of water. At 25 °C, the density of water is 0.9971 g/cm3 and the vapor pressure is 23.76 torr.
3.7 torr
20.06 torr
10.6 torr
12 torr
Using Raoult's law, Psoln = XH2O PH2O
to find the mole fraction of H2O, we have to find the number of moles .
Moles of ethanol = 235/46 = 5.108 mol
Mass of water = volume*density = 500*0.9971 = 498.55 g
Moles of water= 498.55/18 = 27.697 mol
XH2O = 27.697/(27.697+5.108) = 0.844
P = 0.844*23.76 = 20.06 torr
Answer:20.06 torr
Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g...
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