   Chapter 12, Problem 66AE

Chapter
Section
Textbook Problem

# The activation energy for some reaction X 2 ( g )   +   Y 2 ( g )   →   2 XY ( g ) is 167 kJ/mol, and ∆E for the reaction is + 28 kJ/mol. What is the activation energy for the decomposition of XY?

Interpretation Introduction

Interpretation: The activation energy and ΔE is given for the formation of 2XY . By using these values, the activation energy for the decomposition of XY is to be determined.

Concept introduction: A certain threshold energy which is necessary for the reaction to occur is called activation energy.

The relationship between the rate constant and activation energy is given by the Arrhenius equation,

k=AeEaRT

The change in energy (ΔE) is the energy difference between reactant and product. The value of ΔE is either positive or negative.

To determine: The activation energy for the decomposition of XY .

Explanation

Given

The activation energy of given forward reaction is 167kJ/mol .

The change in energy ΔE for forward reaction is 28kJ/mol .

The given reaction is,

X2(g)+Y2(g)2XY(g) .

It is a forward reaction.

The reaction of decomposition of XY is,

2XY(g)X2(g)+Y2(g)

It is a backward reaction.

Formula

The change in energy is calculated by using the formula,

ΔE=Ea(forward)Ea(backward)

Where,

• ΔE is change in energy.
• Ea(forward) is activation energy of forward reaction

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