3 PHASE DIAGRAMS.Sketch the temperature-composition (“T-x") phase diagram for acetone, (CH3)2 CO), and chlo-roform, CHCl3, mixtures based on the following data-⚫ Boiling point(Bp) of pure acetone: 56.2°C•••Bp of pure chloroform: 61.2°CBp of the acetone-chloroform azeotrope: 64.7°CComposition of the azeotrope, by weight: 21% acetone, 79% chloroformAtomic weights (in g mol¯¹): H: 1.010, C: 12.01, O: 16.00, Cl: 35.45Plot the mole fraction of acetone, CHCl 3 on the x-axisOn your sketch of the phase diagram determine the composition of the vapour phase and theliquid phase for a system at 61.2°C having an overall acetone mole fraction of ZA = 0.80.

To sketch the temperature-composition (T-x) phase diagram for the acetone-chloroform mixture, we…

Answered: 3 PHASE DIAGRAMS. Sketch the…

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...

See similar textbooks

Similar questions

For an ethanol-chloroform mixture at 545 mmHg, determine: a) The Liquid - Vapor equilibrium diagram (1pt) b) Boiling temperature with 20% mass of ethanol (1pt) c) The composition of a mixture that has gone through two distillation stages (1pt)
The ΔH°soln of HNO3 is –33.3 kJ/mol. 11.0 mL of 14.0 M HNO3 is dissolved in 100.0 mL of distilled water initially at 25°C. How much ice at 0°C [cP = 37.1 J/(mol ·°C), ΔH°fus = 6.01 kJ/mol] must be added to return the solution temperature to 25°C after dissolution of the acid and equilibrium with the ice is reached? The molar heat capacity is 80.8 J/(mol·°C) for the solution, and the molar heat capacity is 75.3 J/(mol·°C) for pure water.
What is the answer.
A coffee cup calorimeter was filled with 100. mL of water (4.181 J-g.C). 1.02 g NaOH(s) was added resulting in a temperature change of 3.7°C. Determine the heat of dissolution for NaOH in kJ/mol. 1) 104 kJ mol1 O 2) 42 kJ mol-1 3) 35 kJ mol1 4) 61 kJ mol-1 5) 87 kJ mol-1
1. Consider the temperature-composition diagram shown below for benzene (bp = 80°C) and toluene (bp = 110°C). For a 80/20 mixture of toluene to benzene answer the following: Temperature (°C) 110 8 95 90 3 80 1 T 1 1 0.2 0.4 0.6 Mole Fraction of Toluene a) At what temperature will the mixture begin to boil (use just approximate values)? b) When the mixture begins to boil, what is the mol % benzene in the vapor? c) What is the boiling point of the liquid formed by condensation of the vapor? 1 0.8 110 100 95 90 85 80
In a binary mixture, the density of ethanol is 0.7880 g cm-3 at 20.00C. Its equilibrium vapor pressure at 20.00C is 40.0 torr. Calculate the change in its chemical potential at this temperature and composition, if its pressure is changed from 40.0 torr to 1 atm. (Hint: recall uj = Gj,m).
şvurular Posta Gönderileri Place a piece of copper in 0 Word ik: Her şey hazır 19° Gözden Geçir Görünüm Yardım When 50 g of phenol is mixed with 50 g of water at 20°C, two phases are formed. from phases one contains 8% phenol by mass and the other contains 72% phenol. The mass of each phase and this Find the masses of the components in the phases. Ne yapmak istediğinizi söyleyin (Ctrl)
coompute with full solution
Suppose the change in temperature solution is -9.84°C (ΔTf=9.84°C ). The unknown solute consists of 0.404g. The mass of the solvent 14.65g of t-Butanol. What is the molar mass of the solute. Assume the solute is organic kfbutanol=9.1°C *kg/mol
When benzene freezes at 5.5°C its density changes from 0.879 g cm−3 to 0.891 g cm−3. Its enthalpy of fusion is 10.59 kJ mol−1. Estimate the freezing point of benzene at 1000 atm. Answer= ???. ??
In a constant-pressure calorimetry experiment, Jiwon and Jisun dissolved 10.0 g of CaCl2 (MM = 110.98 g mol-1) in 250.0 g of water initially at 20.00°C. As the solid dissolves in water, the temperature rises to 26.73°C. Calculate the enthalpy of dissolution (ΔHdissolution) of CaCl2 in kJ mol-1. Assume that the calorimeter absorbed a negligible amount of heat.
Water and acetonitrile, CH3CN, are miscible (can be mixed in any proportions). However, when water and acetonitrile are mixed, the volumes are not additive (the total volume of the resulting solution is not equal to the sum of the pure liquid volumes). For example, when 100.0 mL of water and 100.0 mL of CH3CN(I), are mixed at 20 °C, the total volume of the solution is 192.0mL, not 200.0 mL. a. Provide an explanation for this phenomenon. b. Calculate the molarity, molality and mol fraction of CH3CN in a solution prepared by mixing 100.0 mL of water and 100.0 mL of CH3CN(1) at 20 °C. The total volume of the mixture is 192.0 mL and the densities of water and acetonitrile are 0.998 g/mL and 0.782 g/mL, respectively, at this temperature. c. When 70.0 g H2O and 190.0 g CH3CN(1) are mixed, to resulting solution has a density of 0.860 g/mL at 20 °C. Calculate the volumes of the pure liquid samples and the solution, and show that the pure liquid volumes are not additive.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS