Worksheet: Electrochemical Cell Potential

In this worksheet, we will practice calculating the potential of an electrochemical cell from the half-cell potentials of the anode and cathode.

Q1:

What is the standard electrode potential for the galvanic cell with the following overall 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 . 7 9 9 6 0 . 4 4 7

Q2:

A galvanic cell consists of a Mg electrode in 1 MMg(NO)32 solution and a Ag electrode in 1 MAgNO3 solution. What is the standard cell potential?

Half-Equation M g ( ) + 2 e M g ( ) 2 + a q s A g ( ) + e A g ( ) + a q s
Standard Electrode Potential, 𝐸 (V) 2 . 3 7 2 + 0 . 7 9 9 6

Q3:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell consisting of Au3+/Au and Ni2+/Ni half-cells.

Half-Equation A u ( ) + 3 e A u ( ) 3 + a q s N i ( ) + 2 e N i ( ) + a q s
Standard Electrode Potential, 𝐸 (V) + 1 . 4 9 8 0 . 2 5 7
  • A 1 . 2 4 1 V
  • B1.755 V
  • C 1 . 7 5 5 V
  • D1.241 V

Q4:

Using the standard electrode potentials in the table below, calculate the standard cell potential 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

Q5:

Using the standard electrode potentials shown in the table, calculate, to 3 decimal places, the cell potential for the following electrochemical cell. Cd()|Cd(,0.10M)Ni(,0.50M)|Ni()saqaqs2+2+

Half-Equation C d ( ) + 2 e C d ( ) 2 + a q s N i ( ) + 2 e N i ( ) 2 + a q s
Standard Electrode Potential, 𝐸()V 0 . 4 0 3 0 0 . 2 5 7
  • A0.167 V
  • B0.146 V
  • C0.164 V
  • D0.155 V
  • E0.125 V

Q6:

Using the standard electrode potentials shown in the table, determine which of the following metals are capable of reducing LaO23 to La metal.

Half-Equation C a ( ) + 2 e C a ( ) 2 + a q s A l ( ) + 3 e A l ( ) 3 + a q s F e ( ) + 2 e F e ( ) 2 + a q s L a ( ) + 3 e L a ( ) 3 + a q s
Standard Electrode Potential, 𝐸 (V) 2 . 8 6 8 1 . 6 6 2 0 . 4 4 7 2 . 5 2
  • A A l only
  • B C a only
  • C F e only
  • D A l and Fe
  • E C a and Al

Q7:

The standard reduction potentials for oxygen gas and two cobalt(III) complexes are shown in the table.

Half-Equation O ( ) + 4 H ( ) + 4 e 2 H O ( ) 2 + 2 g a q l [ C o ( H O ) ] ( ) + e [ C o ( H O ) ] ( ) 2 6 3 + 2 6 2 + a q a q [ C o ( N H ) ] ( ) + e [ C o ( N H ) ] ( ) 3 6 3 + 3 6 2 + a q a q
Standard Electrode Potential, 𝐸()V + 1 . 2 2 9 + 1 . 8 + 0 . 1

Based on the cell potentials, which of the two complexes, [Co(HO)]262+ and [Co(NH)]362+, can be oxidized to the corresponding cobalt(III) complex by oxygen? Assume that all reactions take place under standard conditions.

  • A [ C o ( N H ) ] 3 6 2 + and [Co(HO)]262+
  • B [ C o ( H O ) ] 2 6 2 + but not [Co(NH)]362+
  • C [ C o ( N H ) ] 3 6 2 + but not [Co(HO)]262+
  • DNeither [Co(HO)]262+ nor [Co(NH)]362+
  • EMore information is needed.

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