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Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373

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Chapter
Section
BuyFindarrow_forward

Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373
Textbook Problem

Consider the decomposition at 25°C of one mole of NOBr gas into NO and Br2 gases. At equilibrium, the concentrations of NOBr, NO, and Br2 gases are 0.0162 M, 0.0011 M, and 0.072 M, respectively.

(a) Write a balanced equation for the reaction.

(b) Calculate K for the reaction at 25°C. (Note that the gases need to be expressed as pressure in atm.)

Interpretation Introduction

(a)

Interpretation:

The balanced chemical equation for the reaction needs to be written

Concept introduction:

A chemical reaction is said to balanced, if there are equal number of atoms of same species in both sides of the reaction arrow that is reactant and product side.

Explanation

The decomposition of 1 mol of NOBr produces NO and Br2 gases, the chemical equation for the reaction can be written as follows:

NOBr(g)NO(g)+Br2(g)

To balance the above reaction, give coefficient ½ to Br2(g)

Interpretation Introduction

(b)

Interpretation:

The value of equilibrium constant for the given reaction at 25 C needs to be determined.

Concept introduction:

The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place.

For a general equilibrium reaction as follows:

A(g)+B(g)C(g)+D(g)

The expression for the equilibrium constant is represented as follows:

K=(PC)(PD)(PA)(PB)

Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.

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