   Chapter 15, Problem 22PS

Chapter
Section
Textbook Problem

The equilibrium constant K for the reactionCO2(g) ⇄ CO(g) + ½ O2(g)is 6.66 × 10−12 at 1000 K. Calculate K for the reaction2 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)

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 