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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

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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




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.

Al(s)|Al3+(aq)||H+(aq)|O2(g)|Pt(s)


Example 6 l.jpg
Example 6

Calculate the cell potential for the

following Galvanic cell at 25°C.

Ni(s)|Ni2+(1.0M)||Sn2+(1.0x10-4M)|Sn(s)


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?







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

cathode.


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?





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