   # The activation energy for the reaction NO 2 ( g ) + CO ( g ) → NO ( g ) + CO 2 ( g ) is 125 kJ/mol, and ∆ E for the reaction is −216 kJ/mol. What is the activation energy for the reverse reaction [NO( g ) + CO 2 ( g ) →+ NO 2 ( g ) + CO( g )]? ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404

#### Solutions

Chapter
Section ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404
Chapter 12, Problem 69E
Textbook Problem
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## The activation energy for the reaction NO 2 ( g )   +  CO ( g )   →  NO ( g )   +  CO 2 ( g ) is 125 kJ/mol, and ∆E for the reaction is −216 kJ/mol. What is the activation energy for the reverse reaction [NO(g) + CO2(g) →+ NO2(g) + CO(g)]?

Interpretation Introduction

Interpretation: The activation energy and ΔE for a reaction is given. By using these values, the activation energy for the given reverse reaction is to be calculated.

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 given reverse reaction.

### Explanation of Solution

Given

The activation energy of given forward reaction is 125kJ/mol .

The change in energy ΔE is 216kJ/mol .

The given reverse reaction is,

NO(g)+CO2(g)NO2(g)+CO(g)

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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