Answer :
The total vapor pressure above the solution is approximately 177.65 torr.
To determine the total vapor pressure above the solution, we can 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.
Let's calculate the mole fraction of each component first:
Mole fraction of A (Xa) = moles of A / total moles of solution
= 1.30 moles / (1.30 moles + 2.00 moles)
= 0.393
Mole fraction of B (Xb) = moles of B / total moles of solution
= 2.00 moles / (1.30 moles + 2.00 moles)
= 0.607
Now, we can calculate the partial pressure of each component:
Partial pressure of A (Pa) = Xa * vapor pressure of A
= 0.393 * 97.6 torr
= 38.33 torr
Partial pressure of B (Pb) = Xb * vapor pressure of B
= 0.607 * 229.5 torr
= 139.32 torr
Finally, the total vapor pressure above the solution is the sum of the partial pressures:
Total vapor pressure = Pa + Pb
= 38.33 torr + 139.32 torr
= 177.65 torr
Therefore, the total vapor pressure above this solution is approximately 177.65 torr.
learn more about Raoult's Law here:
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