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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 °C.

Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s)

  1. a. Write a balanced equation for the reaction that occurs at the cathode.
  2. b. Write a balanced equation for the reaction that occurs at the anode.
  3. c. Write a balanced chemical equation for the overall reaction.
  4. d. Determine the potential (in volts) of the cell.

a.

Interpretation Introduction

Interpretation:

Assuming the folloing electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and  25o C.

Zn | Zn(OH)2(s) | OH-(aq) || Cu(OH)2(s) | Cu(s)

A balanced equation for the reaction that occurs at the cathode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Electrolysis:

It is a decomposition of ionic compounds by passing electricity through molten compounds or aqueous solutions of compounds.

Electricity used to produce chemical changes. The apparatus used for electrolysis is called an electrolytic cell.

Generally, oxidation occurs at anode and reduction occurs a cathode.

Explanation

The given voltaic cell representation is as follows.

Zn | Zn(OH)2(s) | OH-(aq) || Cu(OH)2(s) | Cu(s)

At cathode, the reduction reaction occurred. Cu(OH)2(s) is reduced to Cu(s)

b.

Interpretation Introduction

Interpretation:

Assuming the folloing electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and  25o C.

Zn | Zn(OH)2(s) | OH-(aq) || Cu(OH)2(s) | Cu(s)

A balanced equation for the reaction that occurs at the anode has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Electrolysis:

It is a decomposition of ionic compounds by passing electricity through molten compounds or aqueous solutions of compounds.

Electricity used to produce chemical changes. The apparatus used for electrolysis is called an electrolytic cell.

Generally, oxidation occurs at anode and reduction occurs a cathode.

c.

Interpretation Introduction

Interpretation:

Assuming the folloing electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and  25o C.

Zn | Zn(OH)2(s) | OH-(aq) || Cu(OH)2(s) | Cu(s)

A balanced equation for the overall reaction has to be determined

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Electrolysis:

It is a decomposition of ionic compounds by passing electricity through molten compounds or aqueous solutions of compounds.

Electricity used to produce chemical changes. The apparatus used for electrolysis is called an electrolytic cell.

Generally, oxidation occurs at anode and reduction occurs a cathode.

d.

Interpretation Introduction

Interpretation:

Assuming the folloing electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and  25o C.

Zn | Zn(OH)2(s) | OH-(aq) || Cu(OH)2(s) | Cu(s)

The potential of the cell has to be determined.

Concept introduction:

Voltaic cell or Galvanic cell:

The device to produce electricity by using chemical reactions. In these divces are redox chemical reactions are occured.

A voltaic cell converts chemical energy into electrical energy.

It consists of two half cells. Each half cell consists of a metal and a solution of a salt of metal. Two half cells are connected by salt bridge.

The chemical reaction in the half cell is an oxidation reduction (redox)reactions.

For example:

Cell diagram of voltaic or galvanic cell is as follows.

                 Salt bridge                        Cu(s)|Cu2+(aq)  ||  Ag+(aq)|Ag(s)____________     ___________                                       Half cell             Half cell

Electrolysis:

It is a decomposition of ionic compounds by passing electricity through molten compounds or aqueous solutions of compounds.

Electricity used to produce chemical changes. The apparatus used for electrolysis is called an electrolytic cell.

Generally, oxidation occurs at anode and reduction occurs a cathode.

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Chapter 19 Solutions

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Sect-19.8 P-19.11CYUSect-19.9 P-1.1ACPSect-19.9 P-1.2ACPSect-19.9 P-1.3ACPSect-19.9 P-2.1ACPSect-19.9 P-2.2ACPSect-19.9 P-2.3ACPSect-19.9 P-2.4ACPSect-19.9 P-2.5ACPCh-19 P-1PSCh-19 P-2PSCh-19 P-3PSCh-19 P-4PSCh-19 P-5PSCh-19 P-6PSCh-19 P-7PSCh-19 P-8PSCh-19 P-9PSCh-19 P-10PSCh-19 P-11PSCh-19 P-12PSCh-19 P-13PSCh-19 P-14PSCh-19 P-15PSCh-19 P-16PSCh-19 P-17PSCh-19 P-18PSCh-19 P-19PSCh-19 P-20PSCh-19 P-21PSCh-19 P-22PSCh-19 P-23PSCh-19 P-24PSCh-19 P-25PSCh-19 P-26PSCh-19 P-27PSCh-19 P-28PSCh-19 P-29PSCh-19 P-30PSCh-19 P-31PSCh-19 P-32PSCh-19 P-33PSCh-19 P-34PSCh-19 P-35PSCh-19 P-36PSCh-19 P-37PSCh-19 P-38PSCh-19 P-39PSCh-19 P-40PSCh-19 P-41PSCh-19 P-42PSCh-19 P-43PSCh-19 P-44PSCh-19 P-45PSCh-19 P-46PSCh-19 P-47PSCh-19 P-48PSCh-19 P-49PSCh-19 P-50PSCh-19 P-51PSCh-19 P-52PSCh-19 P-53PSCh-19 P-54PSCh-19 P-55PSCh-19 P-56PSCh-19 P-57GQCh-19 P-58GQCh-19 P-59GQCh-19 P-60GQCh-19 P-61GQCh-19 P-62GQCh-19 P-63GQCh-19 P-64GQCh-19 P-65GQCh-19 P-66GQCh-19 P-67GQCh-19 P-68GQCh-19 P-69GQCh-19 P-70GQCh-19 P-71GQCh-19 P-72GQCh-19 P-73GQCh-19 P-74GQCh-19 P-75GQCh-19 P-76GQCh-19 P-77GQCh-19 P-78GQCh-19 P-79GQCh-19 P-80GQCh-19 P-81GQCh-19 P-82GQCh-19 P-83GQCh-19 P-84GQCh-19 P-85GQCh-19 P-86GQCh-19 P-87GQCh-19 P-88GQCh-19 P-89GQCh-19 P-90GQCh-19 P-91GQCh-19 P-92GQCh-19 P-93GQCh-19 P-94GQCh-19 P-95GQCh-19 P-96GQCh-19 P-97GQCh-19 P-98GQCh-19 P-99GQCh-19 P-100GQCh-19 P-101GQCh-19 P-102GQCh-19 P-103GQCh-19 P-104GQCh-19 P-105ILCh-19 P-106ILCh-19 P-107ILCh-19 P-108ILCh-19 P-109ILCh-19 P-110ILCh-19 P-111SCQCh-19 P-112SCQCh-19 P-113SCQCh-19 P-114SCQCh-19 P-115SCQ

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