# 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?

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 | ||
---|---|---|

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 | ||
---|---|---|

Standard Electrode Potential, (V) |

- A V
- B1.755 V
- C 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.

Half-Equation | ||
---|---|---|

Standard Electrode Potential, (V) |

**Q5: **

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

Half-Equation | ||
---|---|---|

Standard Electrode Potential, |

- 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 to metal.

Half-Equation | ||||
---|---|---|---|---|

Standard Electrode Potential, (V) |

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

**Q7: **

The figure shows the setup of a voltaic cell.

What one of the following is the correct expression of the setup in cell notation?

- A
- B
- C
- D
- E

**Q8: **

Concentrated hydrochloric acid is not used to acidify the dichromate ions in the oxidation of a primary alcohol to a carboxylic acid. In practice, the dichromate oxidizes the chloride ions, so sulfuric acid is used instead.

The half-equations and standard electrode potentials for this oxidation are shown:

What would the standard cell potential for a galvanic cell consisting of these two half-cells be?

Is the reaction feasible according to previous calculation? How does this explain the choice of acid in the experiment discussed?

- AThe reaction is feasible and concentrated hydrochloric acid would have a more negative electrode potential (), making the oxidation of chloride ions by dichromate ions also feasible.
- BThe reaction is not feasible; however, concentrated hydrochloric acid would have a more negative electrode potential (), making the oxidation of chloride ions by dichromate ions feasible.
- CThe reaction is feasible and concentrated hydrochloric acid would have a more positive electrode potential (), making the oxidation of chloride ions by dichromate ions also feasible.
- DThe reaction is not feasible; however, concentrated hydrochloric acid would have a more positive electrode potential (), making the oxidation of chloride ions by dichromate ions feasible.