Chapter 17: Electrochemistry - PowerPoint PPT Presentation

Chapter 17 electrochemistry l.jpg
1 / 25

  • Uploaded on
  • Presentation posted in: General

Chapter 17: Electrochemistry. Review of Redox Reactions Galvanic Cells: Using spontaneous redox reactions to generate electrical energy. Galvanic Cells Cell potential D G and work Cell potential and concentration Applications: Batteries, fuel cells, corrosion

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.

Download Presentation

Chapter 17: Electrochemistry

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript

Chapter 17 electrochemistry l.jpg

Chapter 17: Electrochemistry

  • Review of Redox Reactions

  • Galvanic Cells: Using spontaneous redox reactions to generate electrical energy.

    • Galvanic Cells

    • Cell potential

    • DG and work

    • Cell potential and concentration

    • Applications: Batteries, fuel cells, corrosion

  • Electrolytic Cells: Using electricity to cause nonspontaneous redox reactions to occur.

    • Electrolytic Cells

    • Applications: Electrolysis of water, electrolysis of mixtures of ions, production of Al, electrorefining, metal plating, electrolysis of NaCl

Example 1 l.jpg

Example 1

Balance the following redox reactions

using the half reaction method.

  • ClO3- + As2S3 Cl- + H2AsO4- + SO42-

  • K2S + KMnO4 S8 + MnO2 + KOH

Figure 17 6 cartoon of atoms reacting l.jpg

Figure 17.6: Cartoon of atoms reacting

Figure 17 5 a standard hydrogen electrode l.jpg

Figure 17.5: A standard hydrogen electrode

Example 2 l.jpg

Example 2

If a standard Cu|Cu2+ electrode is

connected to a standard Al|Al3+

electrode, what reaction occurs? What

is °cell? Sketch the cell, label the

cathode and anode, show the direction

of electron flow, and give the line

notation for the cell.

Example 3 l.jpg

Example 3

Consider the following species under

standard conditions:

Ce4+, Ce3+, Fe2+, Fe3+, Fe, Mg, Mg2+, Ni2+, Sn

  • Which is the strongest oxidizing agent?

  • Which is the strongest reducing agent?

  • Will Fe dissolve in 1.0 M Ce4+? If so, will Fe3+ or Fe2+ be formed?

  • Which can be oxidized by H+(aq)?

  • Which can be reduced by H2(g)?

Example 4 l.jpg

Example 4

Select an oxidizing agent to oxidize Cl-

to Cl2 without oxidizing Br- to Br2.

Example 5 l.jpg

Example 5

Calculate the maximum work available

from 25.0 g of aluminum in the

following galvanic cell for which the emf

is 1.15 V. Note that O2 is reduced to

H2O in this reaction.


Example 6 l.jpg

Example 6

Calculate the cell potential for the

following Galvanic cell at 25°C.


Example 7 l.jpg

Example 7

Find the potential of a

Ag+(1.0x10-7M)|Ag(s) electrode at 25°C.

Example 8 l.jpg

Example 8

Calculate the equilibrium constant for

the following reaction at 25°C.

Ag+(aq) + Fe2+(aq)  Ag(s) + Fe3+(aq)

Example 9 l.jpg

Example 9

A concentration cell is made up of two

Ag/Ag+ half cells. In the first half cell,

[Ag+] = 0.010 M. In the second half

cell, [Ag+] = 4.0 x 10-4 M. What is the

cell potential? Which half cell functions

as the anode?

Figure 17 13 lead storage battery l.jpg

Figure 17.13: Lead storage battery

Figure 17 14 common dry cell battery l.jpg

Figure 17.14: Common dry cell battery


Figure 17 16 hydrogen oxygen fuel cell l.jpg

Figure 17.16: hydrogen-oxygen fuel cell

Figure 17 17 corrosion of iron l.jpg

Figure 17.17: Corrosion of Iron

Figure 17 18 cathodic protection of an underground pipe l.jpg

Figure 17.18: Cathodic protection of an underground pipe

Example 10 l.jpg

Example 10

Predict the products and calculate the

minimum voltage required for the

electrolysis of the following substances

using platinum electrodes.

  • MgBr2(l)

  • 1.0 M NiCl2(aq)

Example 11 l.jpg

Example 11

Write the net ionic equation for the

reaction you expect to occur when the

electrolysis of NiSO4(aq) is conducted

using a nickel anode and an iron


Example 12 l.jpg

Example 12

How many grams of silver are deposited

at a platinum cathode in the

electrolysis of an aqueous solution of

AgNO3 by 1.73A of electric current in

2.5 hours?

Example 13 l.jpg

Example 13

How long will it take to produce 10.0 g

of bismuth (Bi) by the electrolysis of a

BiO+ solution using a current of 25.0 A?

Figure 17 22 production of al l.jpg

Figure 17.22: Production of Al

Figure 17 23 refining of copper l.jpg

Figure 17.23: Refining of Copper

Figure 17 25 downs cell for production of sodium and chlorine l.jpg

Figure 17.25: Downs cell for production of sodium and chlorine

  • Login