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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)

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)

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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
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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)

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
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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