   # The net reaction that occurs in a voltaic cell is Zn(s) + 2 Ag + (aq) → Zn 2+ (aq) + 2 Ag(s). Calculate a potential for the cell assuming standard conditions. (a) 1562 V (b) 0.0360 V (c) 2361V ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 19.4, Problem 1RC
Textbook Problem
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## The net reaction that occurs in a voltaic cell is Zn(s) + 2 Ag+ (aq) → Zn2+ (aq) + 2 Ag(s). Calculate a potential for the cell assuming standard conditions. (a) 1562 V (b) 0.0360 V (c) 2361V

Interpretation Introduction

Interpretation: The potential for the cell under standard conditions is to be determined from the given option.

Concept introduction:

• The substance that easily be reduced in a reaction is represented as an oxidizing agent. For metal cations, a good oxidizing agent can be determined by the standard reduction potential values.
• Half-cell: In the electrochemical cell, both oxidation and reduction occurs. Oxidation occurs at the anode and reduction occurs at the cathode
• Standard electrode potential of cell is defined as the difference of reduction potential at cathode to the reduction potential at anode.
• For the cathode and anode reactions, the values are taken from the standard reduction potential table. The standard cell potential is calculated by taking the difference between the standard reduction potential values of the cathode and anode.

Ecell0=Ecathode0Eanode0

### Explanation of Solution

Reason for correct option

There are two half-cell reactions are involved

At anode,

Zn(s)Zn2+(aq)+2e Eanode0=0.799V

At cathode,

2Ag+(aq)+2e2Ag(s) Ecathode0=0.763V

Given,

From standard reduction potential table,

Eanode0=EZn2+/Zn0=0.799V

Ecathode0=EAg+/Ag0=0

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