The vapor pressures of CCl4 (A) and C₂HC 3 (B) between 7 = 350 and 360 K, can be determined empirically by the formulas In PA* 2790.78 = 9.2199 1 bar PB (T - 46.75) * 2345.4 In bar = 8.3922 (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. 2 (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 C₂HC 3 (B) between 7 = 350 and 360 K, can be determined empirically by the formulas In PA* 2790.78 = 9.2199 1 bar PB (T - 46.75) * 2345.4 In bar = 8.3922 (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. 2 (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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.83QE
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