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ChemistryIntroductory Chemistry: A Foundation9th Edition

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Chapter 9, Problem 54QAP
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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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If steel wool (iron) is heated until it glows and is placed in a bottle containing pure oxygen, the iron reacts spectacularly to produce iron(III) oxide.

msp;  Fe ( s ) + O 2 ( g ) → Fe 2 O 3 ( s )

1.25 g of iron is heated and placed in a bottle containing 0.0204 mole of oxygen gas, what mass of iron(III) oxide is produced?

Interpretation Introduction

Interpretation:

The mass of iron (III) oxide produced should be calculated.

Concept Introduction:

The expected or theoretical yield of the product depends on the limiting reactant of the reaction. Limiting reactant is the reactant that limits the mass of product formed in the reaction.

Explanation

The balanced chemical equation is as follows:

4Fe(s)+3O2(g)→2Fe2O3(s)

To calculate the mass of iron (III) oxide, limiting reactant should be calculated first.

Calculate the number of moles of Fe and oxygen gas as follows:

Mass of iron is 1.25 g and molar mass is 55.845 g/mol thus, number of moles will be:

n=mM

Putting the values,

n=1.25 g55.845 g/mol=0.0224 mol

From the balanced chemical reaction, 4 mol of Fe produces 2 mol of iron (III) oxide or 1 mol of Fe produces 0.5 mol of iron (III) oxide thus, 0.0224 mol of Fe will give 0.0224×0.5=0.0112 mol of iron (III) oxide

Molar mass of iron (III) oxide is 159.69 g/mol thus, mass can be calculated as follows:

m=n×M

Putting the values,

m=(0

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Sect-9.2 P-9.1SCSect-9.3 P-9.2SCSect-9.3 P-9.3SCSect-9.3 P-1CTSect-9.3 P-9.4SCSect-9.3 P-9.5SCSect-9.5 P-9.6SCSect-9.6 P-9.7SCCh-9 P-1ALQCh-9 P-2ALQ
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