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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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Section
BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 14, Problem 19E
Textbook Problem
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Explain with the help of chemical equations why keeping iron dry prevents it from rusting.

Interpretation Introduction

Interpretation:

The given statement is to be explained, using chemical equation,

Concept Introduction:

Oxidation is the addition of an electronegative element or the removal of an electropositive element in a chemical reaction.

Reduction is the addition of an electropositive element or the removal of an electronegative element in a chemical reaction.

The chemical reaction in which oxidation process and reduction process take place simultaneously, is called a redox reaction.

An oxidizing agent is a substance that has the capacity to oxidize another substance and get reduced in a chemical reaction.

A reducing agent is a substance that has the capacity to reduce another substance and get oxidized in a chemical reaction.

The rusting of iron requires conduction of electrons and is an oxidation-reduction reaction.

Explanation of Solution

The formation of the rust requires iron, oxygen, and water. Rusting occurs when the metal is exposed to moist air.

The oxidation of solid iron is as follows:

FeFe2++2e

The electrons produced by this reaction combine with the hydrogen ions and oxygen, to form water.

Fe2++4e+4H++O22H2O(l)

The ferrous ion combines with the hydroxide ion to form hydrated iron oxide iron. Fe(OH)2 is the green rust.

Fe2+(aq)+2OH(aq)Fe(OH)2(s)

The ferrous ion combines with the hydronium ion and oxygen to form Fe3+

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Chapter 14 Solutions

Chemistry In Focus
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