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3.3 Types of chemical reactions

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Question 19

A student mixes iron with a solution containing silver ions. The changes involving the iron and silver are represented by these half-equations:

SubstanceHalf-equation
IronFe(s)→Fe2+(aq)+2e−\mathrm{Fe(s) \rightarrow Fe^{2+}(aq) + 2e^-}Fe(s)→Fe2+(aq)+2e−
SilverAg+(aq)+e−→Ag(s)\mathrm{Ag^+(aq) + e^- \rightarrow Ag(s)}Ag+(aq)+e−→Ag(s)

State which species is oxidised and which species is reduced. Explain why the oxidised species is the reducing agent.

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3.3 Types of chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /3.3 Types of chemical reactions

112 exam-style questions on OCR GCSE Chemistry 3.3 Types of chemical reactions, covering 3.3.1 Oxidation and reduction in terms of oxygen, 3.3.2 Acids, alkalis and neutralisation, 3.3.3 The pH scale and measuring pH, 3.3.4 Oxidation and reduction in terms of electrons, 3.3.5 Dilute and concentrated, weak and strong acids, and 3.3.6 Hydrogen ion concentration and pH. Each one has a worked solution and a mark scheme showing where the marks go.

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