Lesson: Cell Potentials and Equilibrium Constants

In this lesson, we will learn how to convert the potential of an electrochemical cell to the change in free energy and equilibrium constant.

Sample Question Videos

  • 09:36

Worksheet: 6 Questions • 1 Video

Q1:

Using the standard electrode potentials in the table, calculate to 2 significant figures the equilibrium constant at 25∘C for the following reaction. 2Ag()+Fe()2Ag()+Fe()+2+aqssaq

Half-Equation A g ( ) + e A g ( ) + – a q s F e ( ) + 2 e F e ( ) 2 + – a q s
Standard Electrode Potential, 𝐸⦵ (V) +0.7996 − 0 . 4 4 7

Q2:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at 25∘C for a galvanic cell with the following overall reaction. Sn()+2Cu()Sn()+2Cu()saqaqaq2+2++

Half-Equation S n ( ) + 2 e S n ( ) 2 + – a q s C u ( ) + e C u ( ) 2 + – + a q a q
Standard Electrode Potential, 𝐸⦵ (V) − 0 . 1 3 7 5 + 0 . 1 5 3

Q3:

Calculate, to 3 significant figures, the value of the reaction quotient for the cell diagram shown. Al()Al(,0.150M)Cu(,0.0250M)Cu()saqaqs|‖|3+2+
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