If the oxidation potential of Mg and Al are +2.37 volts and + 1.66 volts respectively, then the Mg would?

Analyze the question: We're given oxidation potentials for Mg (+2.37 V) and Al (+1.66 V). We need to decide whether Mg can displace Al from a solution of its salt.

Concept: The electrochemical (reactivity) series ranks metals by how readily they lose electrons.

• A higher oxidation potential means the metal loses electrons more easily, so it is a stronger reducing agent and more reactive.
• A more reactive metal displaces a less reactive metal from its salt solution.

Solution:

1. Compare the potentials: Mg (+2.37 V) > Al (+1.66 V), so Mg is more reactive than Al.
2. Mg therefore oxidizes more readily than Al.
3. Write the half-reactions: • Mg → Mg²⁺ + 2e⁻ (E° oxidation = +2.37 V) • Al³⁺ + 3e⁻ → Al (reduction, E° = −1.66 V)
4. Overall reaction: 3Mg + 2Al³⁺ → 3Mg²⁺ + 2Al
5. Cell potential = +2.37 + (−1.66) = +0.71 V. A positive value means the reaction is spontaneous.

So Mg will displace Al from a solution of Al³⁺ ions.

Checking the options:

• A. Not replace Al: wrong, since the reaction is spontaneous.
• B. Be replaced by Al: wrong, because Al is less reactive.
• C. Remain in the solution: doesn't make sense, because Mg is a solid metal, and it would actually dissolve as Mg²⁺.
• D. Replace Al: correct.

Tip: In displacement questions, compare oxidation potentials. The metal with the higher oxidation potential is the one that displaces the other. If you are given reduction potentials instead, the metal with the more negative value is the more reactive one. A positive overall cell potential means the reaction goes.