An ideal solution contains 40 mole % of A and 60 mole % of B at 80 degrees C. The vapor pressure of pure A and B at this temp are 480 torr and 890 torr. Calculate the vapor pressure of the solution.

PA = XA*PoA.

PB = XB*PoB.

Ptotal = PA + PB

A = 40 mole percent = 0.40 = XA

B = 60 mole percent = 0.60 = XB

To calculate the vapor pressure of the solution, we need to use Raoult's law, which states that the vapor pressure of a component in an ideal solution is equal to the mole fraction of that component multiplied by its vapor pressure in its pure state.

First, we need to calculate the mole fraction of each component in the solution:

Mole fraction of A = 40 mole % = 0.4
Mole fraction of B = 60 mole % = 0.6

Next, we need to calculate the vapor pressure of each component in the solution using Raoult's law:

Vapor pressure of A in the solution = Mole fraction of A * Vapor pressure of A
= 0.4 * 480 torr

Vapor pressure of B in the solution = Mole fraction of B * Vapor pressure of B
= 0.6 * 890 torr

Finally, the vapor pressure of the solution is the sum of the individual vapor pressures of A and B:

Vapor pressure of the solution = Vapor pressure of A in the solution + Vapor pressure of B in the solution

Now you can substitute the values into the formula and calculate the vapor pressure of the solution.