Zinc reacts with aqueous silver ions. The half equations are:
Zn(s)→Zn2+(aq)+2e−\text{Zn}(s) \rightarrow \text{Zn}^{2+}(aq) + 2\text{e}^{-}Zn(s)→Zn2+(aq)+2e−
Ag+(aq)+e−→Ag(s)\text{Ag}^{+}(aq) + \text{e}^{-} \rightarrow \text{Ag}(s)Ag+(aq)+e−→Ag(s)
Explain which species is oxidised and which species is reduced.
Give the balanced ionic equation for the reaction.
86 exam-style questions on AQA GCSE Chemistry 4.1 Reactivity of metals, covering 4.1.1 Metal oxides, 4.1.2 The reactivity series, 4.1.3 Extraction of metals and reduction, and 4.1.4 Oxidation and reduction in terms of electrons. Each one has a worked solution and a mark scheme showing where the marks go.