Question detail
If the standard electrode potential of a half-cell is -0.76 V, what does this indicate about its ability to act as an oxidizing agent?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Electrode potentials and electrochemical cells (A-level only)
Question
- A. It is a weak oxidizing agent.
- B. It is a strong oxidizing agent.
- C. It cannot act as an oxidizing agent.
- D. It is a strong reducing agent.
Answer
It is a weak oxidizing agent.
Explanation
The correct option is It is a weak oxidizing agent.. It is a weak oxidizing agent. is the best answer because it directly supports the AQA A-Level Chemistry objective to define standard electrode potential. This reasoning is anchored to Standard electrode potentials (A-level only) in Electrode potentials and electrochemical cells (A-level only), and it separates electrode potential from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
Common mistake
Misunderstanding Standard Electrode Potential
Students often confuse standard electrode potential with cell potential, thinking they are the same concept.
To clarify, remember that standard electrode potential (E°) refers to the potential of a half-cell compared to the standard hydrogen electrode, while cell potential (E_cell) is the difference between the standard electrode potentials of the two half-cells in an electrochemical cell. Use the formula E_cell = E°(cathode) - E°(anode) to calculate cell potential. For example, if E°(cathode) = +0.76 V and E°(anode) = -0.44 V, then E_cell = 0.76 V - (-0.44 V) = 1.20 V. Thus, the cell potential is 1.20 V. Keep the correction anchored to Standard electrode potentials (A-level only) and the objective: Define standard electrode potential.
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