   Chapter 15, Problem 1PS

Chapter
Section
Textbook Problem

Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) ⇄ 2 H2O(g) + O2(g) (b) CO(g) + ½ O2g ⇄ CO2(g) (c) C(s) + CO2(g) ⇄ 2 CO(g) (d) NiO(s) + CO(g) ⇄ Ni(s) + CO2(g)

(a)

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

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

The equilibrium constant for the reaction is given below,

Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2

Explanation

The equilibrium constant for the reaction can be calculated as,

2H2O2(g)2H2O(g)+O2(g)

The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.

The equilibrium constant for the above reaction is given below,

Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2

(b)

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

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

The equilibrium constant for the reaction is given below,

Kc=[CO2][CO][O2]1/2Kp=(CO2)(CO)(O2)1/2

Explanation

The equilibrium constant for the reaction can be calculated as,

CO(g)+1/2O2(g)CO2(g)

The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.

The equilibrium constant for the above reaction is given below,

Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2

(c)

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

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

The equilibrium constant for the reaction is given below,

Kc=[CO]2[C][CO2]Kp=(CO)2(C)(CO2)

Explanation

The equilibrium constant for the reaction can be calculated as,

C(s)+CO2(g)2CO(g)

The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.

The equilibrium constant for the above reaction is given below,

Kc=[CO]2[C][CO2]Kp=(CO)2(C)(CO2)

(d)

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

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

The equilibrium constant for the reaction is given below,

Kc=[Ni][CO2][NiO][CO]Kp=(Ni)(CO2)(NiO)(CO)

Explanation

The equilibrium constant for the reaction can be calculated as,

NiC(s)+CO(g)Ni(s)+CO2(g)

The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.

The equilibrium constant for the above reaction is given below,

Kc=[Ni][CO2][NiO][CO]Kp=(Ni)(CO2)(NiO)(CO)

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