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?

Half-equation | ||
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Standard electrode potential, (V) |

**Q2: **

A galvanic cell consists of a electrode in 1 M solution and a electrode in 1 M solution. What is the standard cell potential?

Half-equation | ||
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Standard electrode potential, (V) |

**Q3: **

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

Half-equation | ||
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Standard electrode potential, (V) |

- A V
- B 1.241 V
- C V
- D 1.755 V

**Q4: **

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell with the overall reaction:

Half-equation | ||
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Standard electrode potential, (V) |

**Q5: **

Using the standard electrode potentials shown in the table, calculate to 3 decimal places the cell potential for the electrochemical cell:

Half-equation | ||
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Standard electrode potential, |

- A 0.125 V
- B 0.146 V
- C 0.155 V
- D 0.167 V
- E 0.164 V

**Q6: **

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

Half-equation | ||||
---|---|---|---|---|

Standard electrode potential, |

- A only
- B only
- C and
- D only
- E and

**Q7: **

The standard reduction potentials for oxygen gas and two cobalt(III) complexes are shown below:

Half-equation | |||
---|---|---|---|

Standard electrode potential, | +1.229 | +1.8 | +0.1 |

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

- ANeither nor
- B but not
- C and
- D but not
- EMore information is needed.