The balanced chemical equation for the reaction between aluminium and copper II sulfate is:2 Al s + 3 CuSO aq Al SO aq + 3 Cu s To identify the type of redox reaction, we need to determine the oxidation states of each element before and after the reaction.In the reactants:- Aluminium Al is in its elemental form, so its oxidation state is 0.- Copper Cu in copper II sulfate has an oxidation state of +2.- Sulfur S in sulfate ion SO has an oxidation state of +6.- Oxygen O in sulfate ion SO has an oxidation state of -2.In the products:- Aluminium Al in aluminium sulfate Al SO has an oxidation state of +3.- Copper Cu is in its elemental form, so its oxidation state is 0.- Sulfur S in sulfate ion SO has an oxidation state of +6 no change .- Oxygen O in sulfate ion SO has an oxidation state of -2 no change .Comparing the oxidation states before and after the reaction, we can see that:- Aluminium Al is oxidized from 0 to +3 loses 3 electrons .- Copper Cu is reduced from +2 to 0 gains 2 electrons .Since one species is oxidized while another is reduced, this reaction is a redox reaction, specifically a single displacement also known as a single replacement reaction. In this case, aluminium displaces copper in the copper II sulfate compound.