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 25C 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
  • A 1 . 4 × 1 0
  • B 8 . 4 × 1 0
  • C 2 . 0 × 1 0
  • D 7 . 2 × 1 0
  • E 1 . 2 × 1 0

Q2:

Using the standard electrode potentials in the table below, calculate to 2 significant figures the equilibrium constant at 25C 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
  • A 8 . 2 × 1 0
  • B 6 . 6 × 1 0
  • C3.5
  • D 0 . 0 3 5 × 1 0
  • E 6 . 4 × 1 0

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+

Q4:

What is the cell potential of the concentration cell shown? Zn()Zn(,0.10M)Zn(,0.50M)Zn()saqaqs||2+2+

Q5:

A concentration cell has the following cell diagram. Zn()Zn()Zn()Zn()saqaqs||2+2+

The cell potential for this cell, 𝐸cell, is 0.10 V at 298 K. Calculate, to 2 significant figures, the value of the reaction quotient, 𝑄.

  • A7.0
  • B 2 . 4 × 1 0
  • C 4 . 1 × 1 0
  • D 2 . 0 × 1 0
  • E49

Q6:

For the concentration cell described by the cell diagram shown, the reaction quotient, 𝑄, is 4.2×10. Calculate, to 2 significant figures, the concentration of Zn2+ at the anode of the cell. Zn()Zn()Zn(,0.50M)Zn()saqaqs||2+2+

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

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