At 20.0°C, the vapor pressure of cyclohexane is 66.9 torr, and that of toluene is 21.1 torr. What is the vapor pressure of a solution?

A. [tex]n_1 = \frac{P_1 \cdot V}{R \cdot T}[/tex]
B. [tex]n_2 = \frac{P_2 \cdot V}{R \cdot T}[/tex]
C. [tex]X_1 = \frac{n_1}{n_1 + n_2}[/tex]
D. [tex]X_2 = \frac{n_2}{n_1 + n_2}[/tex]

Question

20-06-2024
Chemistry

High School

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At 20.0°C, the vapor pressure of cyclohexane is 66.9 torr, and that of toluene is 21.1 torr. What is the vapor pressure of a solution?

A. [tex]n_1 = \frac{P_1 \cdot V}{R \cdot T}[/tex]
B. [tex]n_2 = \frac{P_2 \cdot V}{R \cdot T}[/tex]
C. [tex]X_1 = \frac{n_1}{n_1 + n_2}[/tex]
D. [tex]X_2 = \frac{n_2}{n_1 + n_2}[/tex]

Answer :

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mahimase56 mahimase56 · Answer 1 · 2023-08-10T03:01:08-04:00

Final answer:

The vapor pressure of a solution of cyclohexane and toluene can be calculated using Raoult's Law and the vapor pressures and mole fractions of the individual components. Without the exact mole fractions, we cannot fully solve this problem.

Explanation:

The question asks you to find the vapor pressure of a solution of cyclohexane and toluene at 20.0°C, given the individual vapor pressures of cyclohexane and toluene. This can be done using Raoult's Law, which states that the vapor pressure of an ideal solution is dependent on the vapor pressure of each component and the mole fraction of each component in the solution. Since the exact composition of the solution is not given, we can express the vapor pressure of the solution (P) as P = X₁P₁ + X₂P₂, where X₁ and X₂ are mole fractions of cyclohexane and toluene respectively, and P₁ and P₂ are the individual vapor pressures of cyclohexane and toluene. In the absence of the exact mole fractions, this formula cannot be fully solved, but it provides a mechanism to estimate the total vapor pressure of the solution. Hemoglobin isn't involved in this question.

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