| Aim | The aim of the experiment is to investigate and compare the reactivity of zinc, iron, copper, and aluminum metals when exposed to different salt solutions, namely zinc sulphate (ZnSO4), copper sulphate (CuSO4), ferrous sulphate (FeSO4), and aluminum sulphate (Al2(SO4)3). The results obtained from the experiment will be used to determine the order of reactivity of these metals, from the most reactive to the least reactive. |
| Materials Required | Zn metal Fe metal Cu metal Al metal ZnSO4(aq) FeSO4(aq) CuSO4(aq) Al2(SO4)3(aq) Test tubes Dropper pipettes |
| Theory | Reactivity series refers to the order of metals based on their relative reactivities towards chemical reagents. This series is determined based on the observation that a more reactive metal displaces a less reactive metal from salt solution, leading to a displacement reaction. For example, when a small amount of zinc is dipped in copper sulphate solution, zinc is displaced from copper sulphate, resulting in a color change from blue to colorless. This indicates that zinc is more reactive than copper. The reactions of aluminium, zinc, iron, and copper with different salt solutions are as follows: Aluminium has the ability to displace zinc, iron, and copper from their respective salt solutions, indicating that it is more reactive than them. Zinc has the ability to displace iron and copper from their respective salt solutions, indicating that it is more reactive than them. Iron has the ability to displace copper from its salt solution, indicating that it is more reactive than copper. No reaction occurs when any of the metals from zinc, iron, aluminium, and copper are placed in an aqueous solution of Al2(SO4)3. Based on the above reactions, the order of reactivity of these metals, from the most reactive to the least reactive, is as follows: Aluminium Zinc Iron Copper |
| Procedure | 1 .Label four test tubes as ZnSO4, FeSO4, CuSO4, and Al2(SO4)3. 2 .Add 5 ml of each salt solution to their respective labeled test tubes. 3 .Take a small piece of Zn metal and place it in the ZnSO4 solution. 4 .Observe the reaction and record any observations. 5 .Repeat steps 3-4 with Fe metal in the FeSO4 solution, Cu metal in the CuSO4 solution, and Al metal in the Al2(SO4)3 solution. 6 .Arrange the metals in decreasing order of reactivity based on the observations. |
| Observations | ZnSO4(aq) + Zn(s) → ZnSO4(aq) + H2(g)The Zn metal dissolves, producing hydrogen gas bubbles and a clear colorless solution. FeSO4(aq) + Fe(s) → FeSO4(aq) + H2(g)The Fe metal dissolves, producing hydrogen gas bubbles and a pale green solution. CuSO4(aq) + Cu(s) → CuSO4(aq)The Cu metal dissolves slowly, forming a pale blue solution and no gas bubbles. Al2(SO4)3(aq) + 2Al(s) → 3Al3+(aq) + 3SO42-(aq)The Al metal reacts quickly, forming a white precipitate of aluminum ions and sulfate ions. |
