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Answer :
The vapor pressure of the solution is 85.4 torr.
To answer this question, we'll first need to calculate the mole fraction of methanol and glycerol in the solution and use it to calculate the vapor pressure of the solution using Raoult's law. Raoult's law is a law of thermodynamics which states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent present in the solution, where the mole fraction is the ratio of the number of moles of a substance to the total number of moles of all the substances present in the solution. Now, let's calculate the mole fraction of methanol and glycerol in the solution.
Number of moles of methanol = 94.3 g / 32.04 g/mol = 2.944
Number of moles of glycerol = 39.2 g / 92.1 g/mol = 0.425
Mole fraction of methanol = 2.944 / (2.944 + 0.425) = 0.874
Mole fraction of glycerol = 0.425 / (2.944 + 0.425) = 0.126
Now, we can use Raoult's law to calculate the vapor pressure of the solution:
P = (mole fraction of methanol) x (vapor pressure of pure methanol)
= (0.874) x (97.7 torr)
= 85.4 torr
Therefore, the vapor pressure of the solution is 85.4 torr.
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