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

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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Question

The vapor pressures of CCl4 (A) and C₂HCl3 (B) between T = 350 and 360 K, can be
determined empirically by the formulas
2790.78
(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 all
proportions.
In
PA*
1 bar
In
PB*
1 bar
9.2199
= 8.3922
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?

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The Gibbs energy of mixing of a regular solution of components A and B is given by Greal = nRT (x Inx +x Inx +ẞXX), where X and X are mix A B B A B the mole fractions of the two components and ẞ is a dimensionless parameter quantifying deviations from ideal behaviour in terms of the relative strength of A-B interactions compared to A-A and B-B interactions. (i) Use a spreadsheet to calculate A Greal/nRT for XA = 0.01, 0.125, mix 0.25, 0.5, 0.75, 0.875 and 0.99 for ẞ= 0, 1 and 3. Report your calculations in a table and, using a labelled plot, determine the numbers of minima in A Greal/nRT as a function of composition and ẞ. mix [3 (ii) For each value of ẞ, predict the number of liquid phases which you would expect for the mixture. Justify your answer in terms of A-B interactions. [
3.
Give typed solution
Looking at the following image of a curve of partial pressures vs mole fractions of the two components A and B of an ideal mixture of liquids that obeys Raoult's Law where pa and pe are the partial pressures of the two liquids A and B respectively and xa and xg are the mole fractions of A and B respectively, which of the following statements is true? PA Pa R S A. The intercepts R and S are representative of the equilibrium vapour pressures of the components A and B respectively B. The intercepts R and S are representative of the equilibrium vapour pressures of the components B and A respectively C. The slopes of the two curves, red and blue, are representative of the equilibrium vapour pressures of the components A and B respectively D. Both (B) and (C) E. The slopes of the two curves, red and blue, are representative of the mole fractions of the components A and B respectively