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Introductory Chemistry: A Foundati...

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

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Consider the oxidation—reduction reaction

Zn ( s ) + Pb 2+ ( a q ) Zn 2 + ( a q ) + Pb ( s )    Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?

Interpretation Introduction

Interpretation:

The galvanic cell should be sketched, the metal ion reduced, oxidized, half reaction takes place at the anode and that on cathode should be determined.

Concept Introduction:

The oxidation and reduction can be identified by change in oxidation state. If oxidation state of atom of an element increases, it undergoes oxidation and if it decreases, it undergoes reduction.

The general oxidation and reduction half reactions are as follows:

AsA+aq+e

Here, As undergoes oxidation to form A+aq with release of 1 electron. The oxidation state of A increases from 0 to 1.

Similarly,

B+aq+eBs

Here, B+aq undergoes reduction to form Bs with addition of 1 electron. The oxidation state of A decreases from 1 to 0.

Explanation

The given oxidation-reduction is as follows:

Zns+Pb2+aqZn2+aq+Pbs

The two half reaction can be obtained as follows:

ZnsZn2+aq..... (1)

And,

Pb2+aqPbs...... (2)

To balance the reaction (1) add 2 electrons to the right thus,

ZnsZn2+aq+2e

Now, reaction (2) can be balanced by adding 2 electrons to the left thus,

Pb2+aq+2ePbs

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