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P9.2 An ideal solution is made up of the volatile liquids A and B, for which P Initially, the pressure is high enough that only the liquid phase is present. As pressure is reduced, the first vapor is observed at a total pressure of 98.5. Torr. Calculate xA. = 120. Torr and P = 70.5 Torr. A

P9.2 An ideal solution is made up of the volatile liquids A and B, for which P Initially, the pressure is high enough that only the liquid phase is present. As pressure is reduced, the first vapor is observed at a total pressure of 98.5. Torr. Calculate xA. = 120. Torr and P = 70.5 Torr. A

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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**P9.2** An ideal solution is made up of the volatile liquids A and B, for which \( P_A^* = 120 \) Torr and \( P_B^* = 70.5 \) Torr. Initially, the pressure is high enough that only the liquid phase is present. As pressure is reduced, the first vapor is observed at a total pressure of 98.5 Torr. Calculate \( x_A \). In this problem, you're tasked with finding the mole fraction (\( x_A \)) of component A in a binary ideal solution, using the given vapor pressures of the pure components and the total pressure at which the first vapor is observed. ### Explanation: - **\( P_A^* \) and \( P_B^* \):** These are the vapor pressures of pure components A and B, respectively. For A, it's 120 Torr, and for B, it's 70.5 Torr. - **Initial State:** The solution is initially only in the liquid phase because the pressure is above the vapor pressures of both components. - **First Vapor Observation:** As the pressure decreases to 98.5 Torr, vapor starts to form. This is the total pressure at which the first vapor bubble appears. - **Objective:** Calculate the mole fraction of A (\( x_A \)) in the liquid phase when the first vapor is observed. This is an application of Raoult's Law, which connects the vapor pressures of individual components with their mole fractions in an ideal solution.
Transcribed Image Text:**P9.2** An ideal solution is made up of the volatile liquids A and B, for which \( P_A^* = 120 \) Torr and \( P_B^* = 70.5 \) Torr. Initially, the pressure is high enough that only the liquid phase is present. As pressure is reduced, the first vapor is observed at a total pressure of 98.5 Torr. Calculate \( x_A \). In this problem, you're tasked with finding the mole fraction (\( x_A \)) of component A in a binary ideal solution, using the given vapor pressures of the pure components and the total pressure at which the first vapor is observed. ### Explanation: - **\( P_A^* \) and \( P_B^* \):** These are the vapor pressures of pure components A and B, respectively. For A, it's 120 Torr, and for B, it's 70.5 Torr. - **Initial State:** The solution is initially only in the liquid phase because the pressure is above the vapor pressures of both components. - **First Vapor Observation:** As the pressure decreases to 98.5 Torr, vapor starts to form. This is the total pressure at which the first vapor bubble appears. - **Objective:** Calculate the mole fraction of A (\( x_A \)) in the liquid phase when the first vapor is observed. This is an application of Raoult's Law, which connects the vapor pressures of individual components with their mole fractions in an ideal solution.
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