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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

The equilibrium constant K for the reaction

CO2(g) ⇄ CO(g) + ½ O2(g)

is 6.66 × 10−12 at 1000 K. Calculate K for the reaction

2 CO(g) + O2(g) ⇄ 2 CO2(g)

Interpretation Introduction

Interpretation: The equilibrium constant of the given reaction is to be calculated.

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 equilibrium constant of the given reaction is calculated.

Given,

  Equilibrium constant at 1000K, K1=6.66×1012

The balanced chemical equation for the first reaction is,

  CO2(g)CO(g)+12O2(g)

The equilibrium constant for the reaction is,’

  K1=[CO][O2]1/2[CO2]=6.66×1012

The balanced chemical equation for the second reaction is

  2CO(g)+O2(g)2CO2(g)

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