Respuesta :
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
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
The vapor pressure of the solution is 20.757 torr.
According to Raoult's law, the vapor pressure can be given by:
Vapor pressure = Mole fraction [tex]\times[/tex] Partial pressure
Density = [tex]\rm \dfrac{Mass}{Volume}[/tex]
Mass = Density [tex]\times[/tex] Volume
Mass of ethanol = 0.789 g/ml [tex]\times[/tex] 33 ml
Mass of ethanol = 26.037 grams
Mass of water = 0.998 g/ml [tex]\times[/tex] 67
Mass of water = 66.866 grams
Moles = [tex]\rm \dfrac{weight}{molecular\;weight}[/tex]
Moles of ethanol = [tex]\rm \dfrac{26.037}{46}[/tex]
Moles of ethanol = 0.566 mol
Moles of Water = [tex]\rm \dfrac{66.866}{18}[/tex]
Moles of water = 3.714 mol
Total moles of solution = Moles of water + Moles of ethanol
Total moles of solution = 3.714 mol + 0.566 mol
Total moles of solution = 4.28 mol
Mole fraction = [tex]\rm \dfrac{moles\;of\;solute}{moles\;of\;solution}[/tex]
Mole fraction of ethanol = [tex]\rm \dfrac{0.566}{4.28}[/tex]
Mole fraction of ethanol = 0.13
Mole fraction of water = [tex]\rm \dfrac{3.714}{4.28}[/tex]
Mole fraction of water = 0.86
Vapor pressure of ethanol = 0.13 [tex]\times[/tex] 43.9
Vapor pressure of ethanol = 5.707 torr
Vapor pressure of water = 0.86 [tex]\times[/tex] 17.5
Vapor pressure of water = 15.05 torr
The vapor pressure of solution = Vapor pressure of ethanol + Vapor pressure of water
The vapor pressure of solution = 5.707 + 15.05 torr
The vapor pressure of solution = 20.757 torr.
The vapor pressure of the solution is 20.757 torr.
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