Lesson: Standard Reduction Potential

In this lesson, we will learn how to use standard reduction potentials to identify the reduction and oxidation reactions in an electrochemical process.

Sample Question Videos

  • 04:27

Worksheet: 3 Questions • 1 Video

Q1:

Using the standard electrode potentials shown in the table, determine which of the following metals is the most prone to corrosion.

Half-Equation A u ( ) + 3 e A u ( ) 3 + a q s F e ( ) + 2 e F e ( ) 2 + a q s F e ( ) + e F e ( ) 3 + 2 + a q a q M g ( ) + 2 e M g ( ) 2 + a q s H g ( ) + 2 e 2 H g ( ) 2 2 + a q l H g ( ) + 2 e H g ( ) 2 + a q l Z n ( ) + 2 e Z n ( ) 2 + a q s
Standard Electrode Potential, 𝐸(V) + 1 . 4 9 8 0 . 4 4 7 + 0 . 7 7 1 2 . 3 7 2 + 0 . 7 9 7 3 + 0 . 8 5 1 0 . 7 6 1 8

Q2:

Using the standard electrode potentials shown in the table, determine which of the following ions is the strongest oxidizing agent in acidic aqueous solutions.

Half-Equation C r O + 1 4 H + 6 e 2 C r + 7 H O 2 7 2 + 3 + 2 M n O + 8 H + 5 e M n + H O 4 + 2 + 2 T i O + 4 H + 2 e T i + 2 H O 2 + 2 + 2
Standard Electrode Potential, 𝐸(V) + 1 . 3 3 + 1 . 5 1 0 . 5 0

Q3:

Iron, the major reactive component of steel, has a standard reduction potential of 0.447 V. Using the standard electrode potentials shown in the table, determine which of the following metals could be used as a sacrificial anode in the cathodic protection of an underground steel storage tank.

Half-Equation C d ( ) + 2 e C d ( ) 2 + a q s A u ( ) + 3 e A u ( ) 3 + a q s N i ( ) + 2 e N i ( ) 2 + a q s A g ( ) + e A g ( ) + a q s Z n ( ) + 2 e Z n ( ) 2 + a q s
Standard Electrode Potential, 𝐸 (V) 0 . 4 0 3 0 + 1 . 4 9 8 0 . 2 5 7 + 0 . 7 9 9 6 0 . 7 6 1 8

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