   Chapter 15, Problem 21PS

Chapter
Section
Textbook Problem

Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO 2 (g) + ½ O 2 (g)  ⇄  SO 3 (g) K 1 2 SO 3 (g)  ⇄  2 SO 2 (g) + O 2 (g) K 2 Which of the following expressions relates K1 to K2? (a) K2 = K12 (b) K22 = K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2 = 1/K12

Interpretation Introduction

Interpretation: The relation between the equilibrium constant for the given two reactions has to be determined from the given option.

Concept introduction:

Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

For a reaction,

aA+bBcC+dD

The equilibrium constant is, K=[C]c[D]d[A]a[B]b

where,

a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

Explanation

The balanced chemical equation for the first reaction is,

SO2(g)+12O2(g)SO3(g)

The equilibrium constant, K for the reaction is,

[SO3][SO2][O2]1/2=K1

The balanced chemical equation for the second reaction is,

2SO3(g)2SO2(g)+O2(g)

The equilibrium constant, K for the reaction is,

[SO2]2[O2][SO3]2=K2([SO2][O2]1/2[SO3])2

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