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Chemistry In Focus

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

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 14, Problem 12E
Textbook Problem
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Explain how an electrochemical cell works. Include the definitions of anode and cathode in your explanation. Why can an electrochemical cell be used to generate electricity?

Interpretation Introduction

Interpretation:

The working principle of an electrochemical cell is to be explained. Anode and cathode are to be defined. The electrochemical cell is used to generate electricity is to be explained.

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 electrochemical cell is also known as a galvanic or voltaic cell.

The electrochemical cell is a type of battery that converts chemical energy into electrical energy.

Explanation of Solution

The electrochemical cell can be made from zinc metals and copper metals with the solution of their nitrate. The oxidation of zinc metal will occur at the anode and the reduction of copper metal will occurs at the cathode. The zinc metal dissolves into the zinc nitrate solution. The zinc metal becomes positively charged from losing the electrons. The copper electrode will be deposited with elemental copper by copper nitrate solution. The cuperous ions present in the solution deposited on copper electrode by gaining electrons. The two half-cells are connected with an external electrical connection. The two solutions are separated by a salt bridge, which allows the ions to complete the circuit. The electrons flow from the anode to cathode. The electrons are transferred from one chemical substance to the other in an electrochemical cell, driven by the redox reaction.

Zn2+ half-cell reaction will occur as oxidation at the anode.

Zn(s)Zn2+(aq)+2e

Cu half-cell reaction will occur as reduction at the cathode.

Cu2+(s)+2eCu(s)

Adding half-cell reactions gives the

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Chapter 14 Solutions

Chemistry In Focus
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