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E^(@) values of Mg^(2+)//Mg is -2.37V, ...

`E^(@)` values of `Mg^(2+)//Mg` is `-2.37V,` of `Zn^(2+)//Zn` is `-0.76V` and `Fe^(2+)// Fe` is - `0.44V`
Which of the statement is correct ?

A

Zn will reduce `Fe^(2+)`

B

Zn will reducing `Mg^(2+)`

C

Mg oxidises Fe

D

Zn oxidises Fe

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem, we need to analyze the standard reduction potentials (E°) provided for the metals and determine which statements regarding their reducing and oxidizing abilities are correct. ### Step-by-Step Solution: 1. **Identify the Given Standard Reduction Potentials:** - For \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} \): \( E° = -2.37 \, \text{V} \) - For \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \): \( E° = -0.76 \, \text{V} \) - For \( \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \): \( E° = -0.44 \, \text{V} \) 2. **Understand the Implications of the E° Values:** - The more negative the E° value, the stronger the reducing agent. This means that: - Magnesium (Mg) is the strongest reducing agent among the three because it has the most negative E° value (-2.37 V). - Zinc (Zn) is the second strongest reducing agent (-0.76 V). - Iron (Fe) is the weakest reducing agent (-0.44 V). 3. **Determine the Reducing and Oxidizing Abilities:** - Since magnesium has the highest negative value, it can reduce both zinc and iron: - \( \text{Mg} \) can reduce \( \text{Fe}^{2+} \) and \( \text{Zn}^{2+} \). - Zinc can reduce iron because it has a more negative E° value than iron: - \( \text{Zn} \) can reduce \( \text{Fe}^{2+} \). - Iron cannot reduce magnesium or zinc because it has the least negative E° value: - \( \text{Fe} \) cannot reduce \( \text{Mg}^{2+} \) or \( \text{Zn}^{2+} \). 4. **Evaluate the Statements:** - **Statement 1:** Zn will reduce Fe\(^{2+}\). **(Correct)** - **Statement 2:** Zn will reduce Mg\(^{2+}\). **(Incorrect)** - **Statement 3:** Mg oxidizes Fe. **(Incorrect)** - **Statement 4:** Zn oxidizes Fe. **(Incorrect)** 5. **Conclusion:** - The only correct statement is that zinc will reduce iron. ### Final Answer: The correct statement is: **Zn will reduce Fe\(^{2+}\)**.
To solve the problem, we need to analyze the standard reduction potentials (E°) provided for the metals and determine which statements regarding their reducing and oxidizing abilities are correct. ### Step-by-Step Solution: 1. **Identify the Given Standard Reduction Potentials:** - For \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} \): \( E° = -2.37 \, \text{V} \) - For \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \): \( E° = -0.76 \, \text{V} \) - For \( \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \): \( E° = -0.44 \, \text{V} \) ...
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Knowledge Check

  • Given E_(Ag^(+)//Ag)^(@)=+0.80 V, E_(Cu^(2+)//Cu)^(@)=+0.34 V, E_(Fe^(3+)//Fe^(2+))^(@)=+0.76 V, E_(Ce^(4+)//Ce^(3+))^(@)=+1.60 V Which of the following statements is not correct ?

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    B
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    C
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    D
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