A solution was prepared by dissolving 92.1 g of iodine, I2, in 800.0 g of chloroform, CHC3. 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 92.1 g of iodine, I2, in 800.0 g of chloroform, CHC3. 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
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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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The mol fraction must equal either 0.103 or 0.363
The boiling point must equal either 62.8 degrees celsius or 64.8 degrees celsius
Transcribed Image Text:A solution was prepared by dissolving 92.1 g of iodine, 12, in 800.0 g of chloroform, CHCI3.
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:Potentially useful or useless data:
Boiling point of pure chloroform = 61.2 °C
Molar mass of pure chloroform = 119.4 g/mol
Boiling point elevation constant (Kp) for chloroform = 3.63°C-m1
Molar mass of lodine = 253.8 g/mol
moles of solute
moles of solution
Formula : mole fraction
%3D
ATh =Kb m
Also, Tâ = T°b + ATB
O Mol fraction = 0.103
Boiling Point = 64.8°C
O Mol fraction = 0.363
Boiling Point = 62.8°C
O Mol fraction = 0.363
Boiling Point = 64.8°C
O Mol fraction = 0.103
Boiling Point = 62.8°C
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