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3.1 Introducing chemical reactions

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Question 3

Molten silver chloride is electrolysed. The table shows the change at each electrode.

ElectrodeStarting speciesProduct
1silver ions, Ag+\mathrm{Ag^{+}}Ag+silver atoms, Ag\mathrm{Ag}Ag
2chloride ions, Cl−\mathrm{Cl^{-}}Cl−chlorine molecules, Cl2\mathrm{Cl_{2}}Cl2​
a.

Write the half equation for the change at electrode 1 and the half equation for the change at electrode 2.

[2]
b.

Combine your two half equations to write the overall ionic equation for the electrolysis.

[1]
Markscheme

3.1 Introducing chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /3.1 Introducing chemical reactions

134 exam-style questions on OCR GCSE Chemistry 3.1 Introducing chemical reactions, covering 3.1.1 Writing formulae and balanced chemical equations, 3.1.2 Formulae of compounds from ions, and state symbols, 3.1.3 Conservation of mass and observed changes in mass, 3.1.4 Half equations and balanced ionic equations, 3.1.5 The mole and the Avogadro constant, and 3.1.6 Stoichiometry, limiting reactants and reacting masses. Each one has a worked solution and a mark scheme showing where the marks go.

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