The vapor pressure of water at 25.0 degrees C is 23.8 torr. Determine the mass of glucose C6H12O6 in g is needed to add to 237.8 g of water to change the vapor pressure to 22.8 torr
We know that from Raoult's law (Po-P)/Po = X
Where
Po = vapor pressure of pure water = 23.8 torr
P = vapor pressure of solution = 22.8 torr
X = mole fraction of the solute = n/(n+n')
n = number of moles of solute(glucose) = mass/molar mass
= m / 180(g/mole)
n' = number of moles of water = mass/molar mass
= 237.8 g/ 18(g/mole)
= 13.21 mole
Plug the values we get (23.8-22.8) / 23.8 = (m/180)/[(m/180)+13.21]
0.042 = m/[m+2377.8]
99.87 + 0.042m = m
0.958 m = 99.87
m = 104.2 g
So the mass of glucose needed is 104.2g
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