Chemistry
Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 15, Problem 19QP

Write the equilibrium constant expressions for K c  and for  K p p, if applicable, for the following reactions:

(a) 2NO 2 ( g )+7H 2 ( g ) 2NH 3 ( g ) + 4 H 2 O ( l ) ( b ) 2ZnS ( s ) + 3 O 2 ( g ) 2ZnO ( s ) + 2SO 2 ( g ) ( c ) C ( s ) + C O 2 ( g ) 2CO ( g ) ( d ) C 6 H 5 C O O H ( a q ) C 6 H 5 COO ( a q ) + H + ( a q )

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

The equilibrium constant expressions for Kc and Kp in each reaction are to be determined.

Concept introduction:

The chemical equilibrium is a state of a chemical reaction when the rate of forward reaction becomes equal to the rate of reverse reaction and the concentration of the products and reactants becomes constant known as equilibrium concentrations.

According to Dalton’s law, the total pressure of the mixture of nonreactive gases is equal to the partial pressure of individual gases. The pressure utilized by the individual gas is called the partial pressure of that gas.

Equilibrium constant is the ratio of the concentration of reactants and products present in the chemical reaction.

For a general reaction: aA+bBcC+dD

The general formula for writing equilibrium expression for the reaction is given as:

KC=[C]ceqm[D]deqm[A]aeqm[B]beqm

Here, KC is the equilibrium constant and C in KC stands for the concentration. [A], [B], [C], and [D] are the equilibrium concentration of reactants A and B and product C and D, respectively.

A and B are reactants, C is products, and x,y, and z are their respective stoichiometric coefficients.

For the general reaction: aA+bBcC+dD

The general formula for writing equilibrium expression for the reaction is given as:

Kp=PCcPDdPAaPBb

Here, p in Kp stands for the pressure. PA,PB,PC,andPD are the equilibrium partial pressure of reactants A and B and products C and D, respectively.

A and B are reactants, C and D are products, and a,b,c, and d are their respective stoichiometric coefficients.

Equilibrium constants of gas phase reaction are written in terms of partial pressures because concentration of gases is directly proportional to partial pressures.

The relationship between KP and KC is given as:

KP=KC(RT)ΔnKc=KP(RT)Δn

Answer to Problem 19QP

Solution:

(a)

Kc=[NH3]2[NO2]2[H2]7

Kp=[PNH3]2[PNO2]2[PH2]7

(b)

Kc=[SO2]2[O2]3

Kp=[PSO2]2[PO2]3

(c)

Kc=[CO]2[CO2]

Kp=[PCO]2[PCO2]

(d)

Kc=[C6H5COO][H+][C6H5COOH]

The Kp expression for the reaction cannot be written as the equilibrium expression does not contain any gases.

Explanation of Solution

a) 2NO2(g)+7H2(g)2NH3(g)+4H2O(l)

The constant expression for the reaction that is applicable only for chemical reactants and products that are in the same section iscalled homogeneous equilibrium. Only gaseous or aqueous species are in equilibrium expression.

In the given reaction, only NO2,H2, and NH3 will appear in the equilibrium expression.

KC=[C]ceqm[D]deqm[A]aeqm[B]beqm

Kc=[NH3]2[NO2]2[H2]7

Here, Kc is the equilibrium constant, [NH3] is the concentration of ammonia, [NO2] is the concentration of NO2, and [H2] is the concentration of H2.

An equilibrium expression contains only gases. The concentration of gases is expressed as partial pressure. The Kp expression for the reaction is as follows:

Kp=PCcPDdPAaPBb

Kp=[PNH3]2[PNO2]2[PH2]7

Here, Kp is the equilibrium constant pressure, [PNH3] is the partial pressure of ammonia, [PNO2] is the partial pressure of NO2, and [PH2] is the partial pressure of H2.

b) 2ZnS(s)+3O2(g)2ZnO(s)+2SO2(g)

The equilibrium expression for the reaction is as follows:

KC=[C]ceqm[D]deqm[A]aeqm[B]beqm

Kc=[SO2]2[O2]3

Here, Kc is the equilibrium constant, [SO2] is the concentration of SO2, and [O2] is the concentration of O2.

The Kp expression for the reaction is as follows:

Kp=PCcPDdPAaPBb

Kp=[PSO2]2[PO2]3

Here, Kp is the equilibrium constant pressure, [PSO2] is the partial pressure of SO2, and [PO2] is the partial pressure of O2.

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

The equilibrium expression for the reaction is applicable for only CO and CO2.

The equilibrium expression for the reaction is as follows:

KC=[C]ceqm[D]deqm[A]aeqm[B]beqm

Kc=[CO]2[CO2]

Here, Kc is the equilibrium constant, [CO] is the concentration of CO, and [CO2] is the concentration of CO2.

The Kp expression for the reaction is as follows:

Kp=PCcPDdPAaPBb

Kp=[PCO]2[PCO2]

Here, Kp is the equilibrium constant pressure, [PCO] is the partial pressure of CO, and [PCO2] is the partial pressure of CO2.

d) C6H5COOH(aq)C6H5COO(aq)+H+(aq)

The equilibrium expression for the reaction is applicable for both reactants and products because both are in homogeneous equilibrium.

KC=[C]ceqm[D]deqm[A]aeqm[B]beqm

Kc=[C6H5COO][H+][C6H5COOH]

Here, Kc is the equilibrium constant, [C6H5COO],[H+] is the concentration of products, and [C6H5COOH] is the concentration of reactant.

The Kp expression for the reaction cannot be written as the equilibrium expression does not contain any gases.

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Chapter 15 Solutions

Chemistry

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