   Chapter 15, Problem 52GQ

Chapter
Section
Textbook Problem

COCl2 decomposes to CO and Cl2 at high temperatures. Kc at 600 K for the reaction is 0.0071.COCl2(g) ⇄ CO(g) + Cl2(g)If 0.050 mol of COCl2 is placed in a 12.5-L flask, what is the total pressure at equilibrium at 600 K?

Interpretation Introduction

Interpretation:

The total pressure for the reaction when decomposition of COCl2 at equilibrium has to be determined

Concept Introduction:

Equilibrium constant in terms of concentration[Kc]: Equilibrium constant can be expressed in terms of concentration.

aA(g)+bB(g)cC(g)+dD(g)Kc=KCc×KDdKAa×KBb

Molarity: It is the number of moles of substance present in a solution of litre.

Molarity =NumberofmolesofsoluteVolumeofsolution(L)

Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

Explanation

Given:

COCl2(g)CO(g)+Cl2(g)Kc=0.0071NumberofmolesofCOCl2=0.050molV=12.5LT=600K

MolarityofCOCl2=NumberofmolesVolumeofsolution=0.050mol12.5L=4×10-3M

Given the reaction:

COCl2(g)CO(g)+Cl2(g)Initialconcentration4×10-300Ifxmolesof COCl2reactFinalconcentration4×10-3-xxx

Equilibrium constant, Kc=[CO][Cl2][COCl2]0

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