   # A blast furnace is used to reduce iron oxides to elemental iron. The reducing agent for this reduction process is carbon monoxide. a. Given the following data: Fe 2 O 3 ( s ) + 3CO ( g ) → 2Fe ( s ) + 3CO 2 ( g ) Δ H ° = − 23 kJ 3Fe 2 O 3 ( s ) + CO ( g ) → 2Fe 3 O 4 ( s ) + CO 2 ( g ) Δ H ° = − 39 kJ Fe 3 O 4 ( s ) + CO ( g ) → 3FeO ( s ) + CO 2 ( g ) Δ H ° = 18 kJ determine Δ H° for the reaction FeO ( s ) + CO ( g ) → Fe ( s ) + CO 2 ( g ) b. The CO 2 produced in a blast furnace during the reduction process actually can oxidize iron into FeO. To eliminate this reaction, excess coke is added to convert CO 2 into CO by the reaction CO 2 ( g ) + C ( s ) → 2CO ( g ) Using data from Appendix 4, determine Δ H° and Δ S° for this reaction. Assuming Δ H° and Δ S ° do not depend on temperature, at what temperature is the conversion reaction of CO 2 into CO spontaneous at standard conditions? ### 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 20, Problem 65E
Textbook Problem
1 views

## A blast furnace is used to reduce iron oxides to elemental iron. The reducing agent for this reduction process is carbon monoxide.a. Given the following data: Fe 2 O 3 ( s )   +  3CO ( g ) →  2Fe ( s )   +  3CO 2 ( g ) Δ H ° =   − 23 kJ 3Fe 2 O 3 ( s )   +  CO ( g ) →  2Fe 3 O 4 ( s )   + CO 2 ( g ) Δ H ° =   − 39 kJ Fe 3 O 4 ( s )   +  CO ( g ) →  3FeO ( s ) + CO 2 ( g ) Δ H ° =  18 kJ determine ΔH° for the reaction FeO ( s )   +  CO ( g ) →  Fe ( s )   +  CO 2 ( g ) b. The CO2 produced in a blast furnace during the reduction process actually can oxidize iron into FeO. To eliminate this reaction, excess coke is added to convert CO2 into CO by the reaction CO 2 ( g )   +  C ( s )   →  2CO ( g ) Using data from Appendix 4, determine ΔH° and ΔS° for this reaction. Assuming ΔH° and ΔS° do not depend on temperature, at what temperature is the conversion reaction of CO2 into CO spontaneous at standard conditions?

(a)

Interpretation Introduction

Interpretation: The answers are to be stated for the given options.

Concept introduction: The expression to calculate ΔH° is,

ΔH°=npΔH°(product)nfΔH°(reactant)

The expression to calculate ΔS° is,

ΔS°=npΔS°(product)nfΔS°(reactant)

A reaction is said to be spontaneous if the value of ΔG° is negative.

To determine: The value of ΔH° for the given reaction.

### Explanation of Solution

Explanation

The value of ΔH° for the given reaction is 11kJ_ .

For the reaction,

Fe2O3(s)+3CO(g)2Fe(s)+3CO2(g)

The value of ΔH° for the reaction is,

ΔH°=23kJ

Multiply the above equation by coefficient 3 on both side.

3Fe2O3(s)+9CO(g)6Fe(s)+9CO2(g) (1)

The value of ΔH° for this reaction is,

ΔH°=23kJ×3=69kJ

For the reaction,

3Fe2O3(s)+CO(g)2Fe(s)+9CO2(g) (2)

The value of ΔH° for the reaction is,

ΔH°=39kJ

For the reaction,

Fe2O3(s)+CO(g)3FeO(s)+CO2(g)

The value of ΔH° for the reaction is,

ΔH°=18kJ

Multiply the above equation by coefficient 2 on both side

(b)

Interpretation Introduction

Interpretation: The answers are to be stated for the given options.

Concept introduction: The expression to calculate ΔH° is,

ΔH°=npΔH°(product)nfΔH°(reactant)

The expression to calculate ΔS° is,

ΔS°=npΔS°(product)nfΔS°(reactant)

A reaction is said to be spontaneous if the value of ΔG° is negative.

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