   Chapter 13, Problem 28PS

Chapter
Section
Textbook Problem

Pure iodine (105 g) is dissolved in 325 g of CCl4 at 65 °C. Given that the vapor pressure of CCl4 at this temperature is 531 mm Hg, what is the vapor pressure of the CCl4-I2 solution at 65 °C? (Assume that I2 does not contribute to the vapor pressure.)

Interpretation Introduction

Interpretation: The vapor pressure of solution has to be identified.

Concept introduction:

Raoult’s law: The vapor pressure of the solvent over the solution Psolvent is proportional to the mole fraction of the solvent. The ideal solution obeys the Raoult’s law.

PsolventχsolventPsolvent,where,Psolventisthevapor pressure of the solvent over the solution,χsolventis mole fraction of solvent in solution, Psolvent is the vapor pressure of the pure solvent.

Explanation

Given data:

Mass of iodine = 105 gMassofCCl4=325gPsolvento=531 mmHg

MolesofIodine=MassMolarmass=105g253.8g/mol=0.414molMolesofCCl4=MassMolarmass=325g153.8g/mol=2

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