Arrange the following metals in the order in which they displace each other from the solution of their salts. Al, Cu, Fe, Mg and Zn.
The order in which the given metals displace each other from the solution of their salts is: Mg > Al > Zn > Fe > Cu.
A metal with a more negative reduction potential can displace metals with less negative (or positive) reduction potentials from their salt solutions. From the standard electrode potential table provided:
- Mg has E° = -2.36 V
- Al has E° = -1.66 V
- Zn has E° = -0.76 V
- Fe has E° = -0.44 V
- Cu has E° = +0.34 V
Since Mg has the most negative reduction potential, it is the strongest reducing agent and can displace all other metals. Cu has the least negative (positive) reduction potential, making it the weakest reducing agent that cannot displace any of the other metals from their salt solutions.
Explanation
The question tests understanding of the electrochemical series and displacement reactions. A metal higher in the reactivity series (more negative E° value) can displace metals below it from their salt solutions because it has a greater tendency to lose electrons (oxidize). The context provides the standard electrode potentials needed to arrange these metals correctly.
Solution Steps
Step 1: Identify the standard electrode potentials from the table - Mg: -2.36V, Al: -1.66V, Zn: -0.76V, Fe: -0.44V, Cu: +0.34V
Step 2: Arrange metals in order of decreasing reducing power (most negative to least negative E° values)
Step 3: Write the final order: Mg > Al > Zn > Fe > Cu