A solution was prepared by dissolving 125.2 g of iodine, I2, in 875.0 g of chloroform, CHCl3. Answer the following questions: 1. Calculate the mole fraction of iodine in the solution. 2. Find the boiling point of the solution. (Hint: iodine is nonvolatile and non-dissociating solid)
A solution was prepared by dissolving 125.2 g of iodine, I2, in 875.0 g of chloroform, CHCl3. Answer the following questions: 1. Calculate the mole fraction of iodine in the solution. 2. Find the boiling point of the solution. (Hint: iodine is nonvolatile and non-dissociating solid)
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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A solution was prepared by dissolving 125.2 g of iodine, I2, in 875.0 g of chloroform, CHCl3.
Answer the following questions:
1. Calculate the mole fraction of iodine in the solution.
2. Find the boiling point of the solution. (Hint: iodine is nonvolatile and non-dissociating solid)
Transcribed Image Text:Boiling point of pure chloroform 61.2 °C
Molar mass of pure chloroform 119.4 g/mol
%D
Boiling point elevation constant (Kp) for chloroform = 3.63°C-m¬1
Molar mass of lodine = 253.8 g/mol
moles of solute
Formula : mole fraction
%3D
moles of solution
ATb = Kb m
Also, T = T°b +ATp
%3D
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