The vapor pressures of CCl4 (A) and C₂HCl3 (B) between T = 350 and 360 K, can be determined empirically by the formulas (₁ In In 7) = PA 1 bar PB* 1 bar = 9.2199 = 8.3922 2790.78 (T-46.75) 2 2345.4 (T-80.45) where T is given in K, and the vapor pressures will be in units of bars. In this problem, assume that these two substances form an ideal solution in this temperature range, in all proportions. (a) Find the mole fraction of CCl4 (component A) in both the liquid and vapor phases at T = 354 K, and an ambient pressure of 0.96 bar. (b) Suppose this mixture is heated slightly to a temperature of T = 358 K but its solution has the same composition (i.e. the same mole fractions of CCl4 and C₂HCl3). What is the total vapor pressure of the solution now (in bars), and what is the mole fraction of CCl4 in the vapor?

The vapor pressures of CCl4 (A) and C₂HCl3 (B) between T = 350 and 360 K, can be determined empirically by the formulas (₁ In In 7) = PA 1 bar PB* 1 bar = 9.2199 = 8.3922 2790.78 (T-46.75) 2 2345.4 (T-80.45) where T is given in K, and the vapor pressures will be in units of bars. In this problem, assume that these two substances form an ideal solution in this temperature range, in all proportions. (a) Find the mole fraction of CCl4 (component A) in both the liquid and vapor phases at T = 354 K, and an ambient pressure of 0.96 bar. (b) Suppose this mixture is heated slightly to a temperature of T = 358 K but its solution has the same composition (i.e. the same mole fractions of CCl4 and C₂HCl3). What is the total vapor pressure of the solution now (in bars), and what is the mole fraction of CCl4 in the vapor?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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