Chlorine reacts with iron(II) ions in solution. The two half equations are:
Fe2+→Fe3++e− \mathrm{Fe^{2+} \rightarrow Fe^{3+} + e^{-}} Fe2+→Fe3++e− Cl2+2e−→2Cl− \mathrm{Cl_{2} + 2e^{-} \rightarrow 2Cl^{-}} Cl2+2e−→2Cl−What is the balanced ionic equation for the overall reaction?
Fe2++Cl2→Fe3++2Cl−\mathrm{Fe^{2+} + Cl_{2} \rightarrow Fe^{3+} + 2Cl^{-}}Fe2++Cl2→Fe3++2Cl−
2Fe2++Cl2→2Fe3++2Cl−\mathrm{2Fe^{2+} + Cl_{2} \rightarrow 2Fe^{3+} + 2Cl^{-}}2Fe2++Cl2→2Fe3++2Cl−
Fe2++Cl→Fe3++Cl−\mathrm{Fe^{2+} + Cl \rightarrow Fe^{3+} + Cl^{-}}Fe2++Cl→Fe3++Cl−
2Fe2++Cl2+2e−→2Fe3++2Cl−\mathrm{2Fe^{2+} + Cl_{2} + 2e^{-} \rightarrow 2Fe^{3+} + 2Cl^{-}}2Fe2++Cl2+2e−→2Fe3++2Cl−
55 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.