Question detail
In the electrolysis of molten NaCl, which half‑equation would you write for the cathode and which for the anode? State the products formed at each electrode.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Electrolysis
Question
In the electrolysis of molten NaCl, which half‑equation would you write for the cathode and which for the anode? State the products formed at each electrode.
Answer
Cathode: Na⁺ + e⁻ → Na (solid). The product is metallic sodium. Anode: 2Cl⁻ → Cl₂(g) + 2e⁻. The product is chlorine gas. The cathode half‑equation shows reduction (gain of electrons) and the anode half‑equation shows oxidation (loss of electrons).
Explanation
This question requires the student to apply the distinction between cathode and anode half‑equations to a specific example, testing application and recall of the reactivity series. It also checks knowledge of the products of molten NaCl electrolysis.
Common mistake
Confusing Cathode and Anode Half Equations
Students often confuse the half equations for the cathode and anode during electrolysis, mistakenly attributing the reduction process to the anode instead of the cathode.
Remember that reduction occurs at the cathode where positive ions gain electrons, while oxidation occurs at the anode where negative ions lose electrons. Practice identifying the charge of ions to help distinguish between the two.
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