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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.

Worksheet • 2 Questions

Q1:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at 2 5 ∘ C for a galvanic cell with the overall reaction:

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
  • A 6 . 6 × 1 0
  • B 6 . 4 × 1 0
  • C 8 . 2 × 1 0
  • D 7 . 4 × 1 0
  • E3.5

Q2:

Using the standard electrode potentials in the table, calculate to 2 significant figures the equilibrium constant at 2 5 ∘ C for the reaction:

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
  • A 1 . 4 × 1 0
  • B 7 . 2 × 1 0
  • C 2 . 0 × 1 0
  • D 8 . 4 × 1 0
  • E 1 . 2 × 1 0
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