Benzene, C6H6, and toluene, C6H5CH3, form an ideal solution. The vapor pressure of benzene is 94.6 Torr and that of Topic 5C Exercises 372 Topic 5C Phase Equilibria in Two-Component Systems toluene is 29.1 Torr at 25 8C. What is the vapor pressure of each component at 25 8C and what is the total vapor pressure of a mix- ture of 1.00 mol benzene and 0.400 mol toluene at 25 8C?

The vapor pressure of benzene and toluene at 25°C is 27.056 torr and 20.777 Torr respectively and the total vapor pressure of mixture is 47.833 Torr

Explanation:

We are given:

Moles of benzene = 1.00 moles

Moles of toluene = 0.400 moles

Mole fraction of a substance is given by:

To calculate the vapor pressure of substance in a mixture, we use the equation given by Raoult's law, which is:

      ........(1)

Using equation 1, we get:

Vapor pressure of pure benzene = 94.6 Torr

Putting values in equation 1, we get:

Using equation 1, we get:

Vapor pressure of pure toluene = 29.1 Torr

Putting values in equation 1, we get:

To calculate the total vapor pressure of the mixture, we use the law given by Dalton, which is:

Hence, the vapor pressure of benzene and toluene at 25°C is 27.056 torr and 20.777 Torr respectively and the total vapor pressure of mixture is 47.833 Torr

a:

by the combination of an unlimited number of elements