   # At a given temperature, K = 1.3 × 10 −2 for the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) Calculate values of K for the following reactions at this temperature. a .· 1 2 N 2 ( g ) + 3 2 H 2 ( g ) ⇌ NH 3 ( g ) b . 2 N H 3 ( g ) ⇌ N 2 ( g ) + 3 H ( g ) c . NH 3 ( g ) ⇌ 1 2 N 2 ( g ) + 3 2 H 2 ( g ) d. 2N 2 ( g ) + 6 H 2 ( g ) ⇌ 4 NH 3 ( g ) ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 23E
Textbook Problem
1 views

## At a given temperature, K = 1.3 × 10−2 for the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) Calculate values of K for the following reactions at this temperature.a.· 1 2 N 2 ( g ) + 3 2 H 2 ( g ) ⇌ NH 3 ( g ) b. 2 N H 3 ( g ) ⇌ N 2 ( g ) + 3 H ( g ) c. NH 3 ( g ) ⇌ 1 2 N 2 ( g ) + 3 2 H 2 ( g ) d. 2N 2 ( g ) + 6 H 2 ( g ) ⇌ 4 NH 3 ( g )

(a)

Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

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 K .

To determine: The equilibrium constant for the given reaction.

### Explanation of Solution

Given

The stated reaction is,

N2(g)+3H2(g)2NH3(g)

The equilibrium constant (K) for the stated reaction is 1.3×102 .

At equilibrium, the equilibrium constant expression is stated,

K=[NH3]2[N2][H2]3

Where,

• K is the equilibrium constant.

The stated reaction is,

12N2(g)+32H2(g)NH3(g)

At equilibrium, the equilibrium constant expression is stated,

K1=[NH3][N2]12[H2]32

Where,

• K1 is the equilibrium constant for this reaction

(b)

Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

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 K .

To determine: The equilibrium constant for the given reaction.

(c)

Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

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 K .

To determine: The equilibrium constant for the given reaction.

(d)

Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

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 K .

To determine: The equilibrium constant for the given reaction.

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