The vapor pressures of CCl4 (A) and C₂HCl3 (B) between T = 350 and 360 K, can bedetermined empirically by the formulas2790.78(T - 46.75)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 allproportions.InPA*1 barInPB*1 bar9.2199= 8.39222(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 hasthe same composition (i.e. the same mole fractions of CCl4 and C₂HCl3). What is the totalvapor pressure of the solution now (in bars), and what is the mole fraction of CCl4 in thevapor?

The objective of the question is to calculate-The mole fraction of in Liquid PhaseThe mole fraction…

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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