   Chapter 15, Problem 34GQ

Chapter
Section
Textbook Problem

The equilibrium constant, Kc, for the following reaction is 1.05 at 350 K.2 CH2Cl2(g) ⇄ CH4(g) + CCl4(g)If an equilibrium mixture of the three gases at 350 K contains 0.0206 M CH2Cl2(g) and 0.0163 M CH4, what is the equilibrium concentration of CCl4?

Interpretation Introduction

Interpretation: The concentration of CCl4 when the system comes to equilibrium should 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.

Explanation

The concentration of CCl4 when the system comes to equilibrium is determined

The balanced equation for the given reaction is,

2CH2Cl2(g)CH4(g)+CCl4(g)

The value of Kc for this reaction is 1.05at350K

The initial concentration of CH2Cl2,CH4 are 0.0206Mand0.0163M respectively.

The equilibrium constant for the reaction can be written as,

K=[CH4][CCl4][CH2Cl2]2

Substituting the known values in the above equation,

1.05=(0

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