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E^(c-) of Mg^(2+)|Mg,Zn^(2+)|Zn, and Fe^...

`E^(c-)` of `Mg^(2+)|Mg,Zn^(2+)|Zn`, and `Fe^(2+)|Fe` are `-2.37V,-0.76V`, and `-0.44V`, respectively. Which of the following is correct ?

A

`Mg^(2+)` oxidises Fe

B

Zn oxidises `Fe^(2+)`

C

Zn reduces `Mg^(2+)`

D

Zn reduces `Fe^(2+)`

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem, we need to analyze the given standard reduction potentials and determine which statements about oxidation and reduction are correct. Let's break it down step by step. ### Step 1: Identify the Standard Reduction Potentials We have the following standard reduction potentials: - \( E^\circ \) for \( Mg^{2+} + 2e^- \rightarrow Mg \) is \(-2.37 \, V\) - \( E^\circ \) for \( Zn^{2+} + 2e^- \rightarrow Zn \) is \(-0.76 \, V\) - \( E^\circ \) for \( Fe^{2+} + 2e^- \rightarrow Fe \) is \(-0.44 \, V\) ### Step 2: Determine the Order of Reduction Potentials The higher (less negative) the reduction potential, the stronger the oxidizing agent. Thus, we can order the metals based on their reduction potentials: 1. \( Fe^{2+} \) (highest reduction potential: \(-0.44 \, V\)) 2. \( Zn^{2+} \) (middle reduction potential: \(-0.76 \, V\)) 3. \( Mg^{2+} \) (lowest reduction potential: \(-2.37 \, V\)) ### Step 3: Identify Oxidizing and Reducing Agents - Since \( Fe^{2+} \) has the highest reduction potential, it can oxidize both \( Zn \) and \( Mg \). - \( Zn \) can oxidize \( Mg \) because it has a higher reduction potential than \( Mg^{2+} \). - \( Mg \) cannot oxidize \( Fe \) or \( Zn \) because it has the lowest reduction potential. ### Step 4: Analyze the Options Now we will evaluate each option based on our findings: 1. **Mg can oxidize Fe**: This is incorrect. \( Fe \) can oxidize \( Mg \), not the other way around. 2. **Zn can oxidize Fe**: This is incorrect. \( Fe \) can oxidize \( Zn \), not the other way around. 3. **Zn can reduce Mg**: This is incorrect. \( Zn \) cannot reduce \( Mg \) because \( Mg \) has a lower reduction potential. 4. **Zn can reduce Fe**: This is correct. \( Zn \) can reduce \( Fe^{2+} \) because it has a higher oxidation potential than \( Fe^{2+} \). ### Conclusion The correct answer is that **Zinc reduces \( Fe^{2+} \)**.
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