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IB Chemistry HL 3.2.16 Electroplating Question Bank

Practise IB Chemistry HL 3.2.16 with questions explaining electroplating, electrode roles and metal-ion reduction at the cathode.

Syllabus
First assessment 2025
Course
Chemistry HL
Level
HL

Exam points

  • connect the object being plated as the cathode where metal ions are reduced
  • identify how the anode or electrolyte maintains the supply of coating-metal ions
  • link fixed current and time to charge, electron amount and the mass of metal deposited

3.2.16 (HL)—Electroplating question 1

[Maximum number: 3]

Iron rusts in the presence of oxygen and water. Rusting is a redox process involving several steps that produces hydrated iron(III) oxide, Fe2O3∙nH2O\mathrm{Fe}_{2} \mathrm{O}_{3} \bullet \mathrm{nH}_{2} \mathrm{O}, as the final product. The half-equations involved for the first step of rusting are given below.

Half-equation 1: Fe(s)→Fe2+(aq)+2e−\quad \mathrm{Fe}(\mathrm{s}) \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-}

Half-equation 2: O2(aq)+4e−+2H2O(l)→4OH−(aq)\quad \mathrm{O}_{2}(\mathrm{aq})+4 \mathrm{e}^{-}+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 4 \mathrm{OH}^{-}(\mathrm{aq})

Describe how electrolysis can be used to electroplate a bracelet with a layer of silver metal. Include the choice of electrodes and electrolyte needed in your description.

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