The vapour pressure of pure benzene and toluene at `40^(@)C` are 184.0 torr and 59.0 torr, respectively. Calculate the partial presure of benzene and toluene, the total vapour pressure of the solution and the mole fraction of benzene in the vapour above the solution that has `0.40` mole fraction of benzene. Assume that the solution is ideal.

Explanation

To solve the problem step by step, we will use Raoult's Law and the information provided about the vapor pressures of pure benzene and toluene.

### Step 1: Identify the given data
- Vapor pressure of pure benzene (P0A) = 184.0 torr
- Vapor pressure of pure toluene (P0B) = 59.0 torr
- Mole fraction of benzene in the solution (XA) = 0.40
- Therefore, mole fraction of toluene (XB) = 1 - XA = 1 - 0.40 = 0.60

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