   Chapter 15, Problem 35GQ

Chapter
Section
Textbook Problem

Carbon tetrachloride can be produced by the following reaction:CS2(g) + 3 Cl2(g) ⇄ S2Cl2(g) + CCl4(g)Suppose 0.12 mol of CS2 and 0.36 mol of Cl2 are placed in a 10.0-L flask. After equilibrium has been achieved, the mixture contains 0.090 mol CCl4. Calculate Kc.

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be determined.

Concept introduction:

• Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. And it is represented by the letter K.

For a general reaction, aA+bBcC+dD

The equilibrium constant Kc=[C]c[D]d[A]a[B]b    a, b, c and d are the stoichiometric coefficients of reactant and product in the reaction. Concentration value for solid substance is 1.

If the value of Kc and the concentration of any of the reactant of a reaction is known then the concentration of product can be determined by multiplying Kc with the concentration of reactant.

• ICE (reaction initial concentration equilibrium) table is mainly used to calculate the value of K for a reaction. This table contains the concentration of reactant and product in various stage of reaction.
• Concentration=AmountofsubstanceVolume
Explanation

The balanced equation for the given reaction is,

CS2(g)+3Cl2(g)S2Cl2(g)+CCl4(g)

The initial concentration of CS2andCl2 are 0.012Mand0.036M.

The equilibrium concentration of CCl4 is 0.009M.

By using these concentration ICE table for this reaction can be constructed.

CS2+3Cl2S2Cl2+CCl4I0.0120.03600Cx3x+x+xE0.012x0

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