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Chemistry & Chemical Reactivity

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

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Chapter
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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

Which of the following correctly relates the two equilibrium constants for the two reactions shown?

NOCl(g) ⇄ NO(g) + ½ Cl2(g)    K1

2 NO(g) + Cl2(g) ⇄ 2 NOCI(g)    K2

  1. (a) K2 = − K 1 2
  2. (b) K2 = 1/(K1)1/2
  3. (c) K2 = 1 / K 1 2
  4. (d) K2 = 2K1

Interpretation Introduction

Interpretation: The correct relation between the two equilibrium constants of the two reactions should be determined from the given options.

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

Reason for the correct answer

The balanced chemical equation for the first reaction is,

  NOCl(g)NO(g)+12Cl2(g)

The balanced chemical equation for the second reaction is,

  2NO(g)+Cl2(g)2NOCl(g)

The equilibrium constant for the first reaction can be written as,

    K1=[NO][Cl2]12[NOCl]

And equilibrium constant for the second re

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