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A solution is composed of 1.60 mol of cyclohexane (P = 97.6 torr) and 2.80 mol of acetone (P = 229.5 torr). What is the total vapor pressure above this solution? Express your answer with the appropriate units.

Answer :

Final answer:

The total vapor pressure above the solution is 181.5 torr.

Explanation:

To find the total vapor pressure above the solution, we need to calculate the partial pressures of cyclohexane and acetone and then sum them up.

First, let's calculate the mole fraction of each component:

Mole fraction of cyclohexane (Xcyclohexane) = moles of cyclohexane / total moles of solution = 1.60 mol / (1.60 mol + 2.80 mol) = 0.3636

Mole fraction of acetone (Xacetone) = moles of acetone / total moles of solution = 2.80 mol / (1.60 mol + 2.80 mol) = 0.6364

Next, let's calculate the partial pressures:

Partial pressure of cyclohexane (Pcyclohexane) = Xcyclohexane * Pcyclohexane = 0.3636 * 97.6 torr = 35.5 torr

Partial pressure of acetone (Pacetone) = Xacetone * Pacetone = 0.6364 * 229.5 torr = 146.0 torr

Finally, we can calculate the total vapor pressure:

Total vapor pressure (Ptotal) = Pcyclohexane + Pacetone = 35.5 torr + 146.0 torr = 181.5 torr

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