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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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?

  1. (a) K2 = K12
  2. (b) K22 = K1
  3. (c) K2 = K1
  4. (d) K2 = 1/K1
  5. (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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