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At 35°C, K = 1.6 × 10 −5 for the reaction 2 NOCl ( g ) ⇌ 2 NO ( g ) + Cl 2 ( g ) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a . 2.0 moles of pure NOCI in a 2.0-L flask b . 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask c . 2.0 moles of NOCI and 1.0 mole of CI 2 in a 1.0-L flask

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 57E
Textbook Problem
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At 35°C, K = 1.6 × 10−5 for the reaction

2 NOCl ( g ) 2 NO ( g ) + Cl 2 ( g )

Calculate the concentrations of all species at equilibrium for each of the following original mixtures.

a. 2.0 moles of pure NOCI in a 2.0-L flask

b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask

c. 2.0 moles of NOCI and 1.0 mole of CI2 in a 1.0-L flask

(a)

Interpretation Introduction

Interpretation: The equilibrium constant value for a decomposition reaction of NOCl is given. The equilibrium concentrations of the species involved in the given reaction are to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented as K .

To determine: The equilibrium concentrations of the species involved in the given reaction.

Explanation of Solution

Given

The stated reaction is,

2NOCl(g)2NO(g)+Cl2(g)

The initial number of moles NOCl is 2.0moles .

The volume of the flask is 2.0L .

The equilibrium constant (K) is 1.6×105 .

The concentration of a reactant is calculated by the formula,

Concentration=MolesVolume(L)

The initial concentration of NOCl is calculated by the formula,

ConcentrationofNOCl=MolesofNOClVolumeoftheflask(L)

Substitute the given values of the number of moles of NOCl and the volume of the flask in the above expression.

ConcentrationofNOCl=2.0mole2.0L=1.0M

The concentration of NOCl consumed is assumed to be 2x .

The equilibrium concentrations are represented as,

2NOCl(g)2NO(g)+Cl2(g)Initialconcentration1.000Change2x+2x+xEquilibriumconcentration1.02x2xx

At equilibrium, the equilibrium ratio is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Where,

  • K is the equilibrium constant.

The equilibrium ratio for the given reaction is,

K=[NO]2[Cl2][NOCl]2 (1)

According to the formulated ICE table,

The equilibrium concentration of NOCl(g) is (1.02x)M .

The equilibrium initial concentration of NO(g) is (2x)M .

The equilibrium initial concentration of Cl2(g) is (x)M .

Substitute these values in equation (1).

K=[NO]2[Cl2][NOCl]2K=[2x]2[x][1

(b)

Interpretation Introduction

Interpretation: The equilibrium constant value for a decomposition reaction of NOCl is given. The equilibrium concentrations of the species involved in the given reaction are to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented as K .

To determine: The equilibrium concentrations of the species involved in the given reaction.

(c)

Interpretation Introduction

Interpretation: The equilibrium constant value for a decomposition reaction of NOCl is given. The equilibrium concentrations of the species involved in the given reaction are to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented as K .

To determine: The equilibrium concentrations of the species involved in the given reaction.

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Chapter 12 Solutions

Chemistry: An Atoms First Approach
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