Worksheet: Cell Potentials and Equilibrium Constants

In this worksheet, we will practice converting the potential of an electrochemical cell to the change in free energy and equilibrium constant.

Q1:

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

Q2:

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
  • A3.5
  • B 8 . 2 × 1 0
  • C 7 . 4 × 1 0
  • D 6 . 6 × 1 0
  • E 6 . 4 × 1 0

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