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Solved: Two liquids A and B have vapor pressures of 76
Chapter 12, Problem 86P(choose chapter or problem)
Two liquids A and B have vapor pressures of 76 mmHg and 132 mmHg, respectively, at 25°C. What is the total vapor pressure of the ideal solution made up of (a) 1.00 mole of A and 1.00 mole of B and (b) 2.00 moles of A and 5.00 moles of B?
Questions & Answers
QUESTION:
Two liquids A and B have vapor pressures of 76 mmHg and 132 mmHg, respectively, at 25°C. What is the total vapor pressure of the ideal solution made up of (a) 1.00 mole of A and 1.00 mole of B and (b) 2.00 moles of A and 5.00 moles of B?
ANSWER:Step 1 of 3
Given that two liquids A and B have vapor pressures of 76 mmHg and 132 mmHg, respectively, at 25°C. We need to find the total vapor pressure of the ideal solution under the two given conditions
(a) 1.00 mole of A and 1.00 mole of B
(b) 2.00 moles of A and 5.00 moles of B
The vapor pressure of the solvent over a solution is given by the product of the vapor pressure of the pure solvent and the mole fraction of the solvent in the solution is stated by Raoult's law.
where and are the partial pressures over the solution for components and
and are the vapor pressures of the pure substances and
and are their mole fractions.