Question

At a certain temperature the vapor pressure of pure benzene (C6H6) is measured to be 204 torr. Suppose a solution is prepared by mixing 50.6 g of benzene and 131 g of acetyl bromide (CH3COBr). What is the partial pressure of benzene vapor above this solution?

A. 56.8 torr
B. 147 torr
C. 204 torr
D. 77.1 torr
E. 127 torr

Answer 1

To calculate the partial pressure of benzene vapor above the solution, we need to use Raoult's law and calculate the mole fraction of benzene in the solution. The partial pressure of benzene vapor above this solution is 56.8 torr (option A).

Step-by-step explanation:

To calculate the partial pressure of benzene vapor above the solution, we need to use Raoult's law and calculate the mole fraction of benzene in the solution. The partial pressure of benzene vapor above this solution is 56.8 torr (option A).

To calculate the partial pressure of benzene vapor above the solution, we need to use Raoult's law, which states that the vapor pressure of a component in a solution is directly proportional to its mole fraction in the solution.

First, we need to calculate the mole fraction of benzene in the solution. We can do this by dividing the moles of benzene by the total moles of both benzene and acetyl bromide.

Next, we can use the mole fraction of benzene to calculate the partial pressure of benzene using the vapor pressure of pure benzene.

The partial pressure of benzene vapor above this solution is 56.8 torr (option A).