Keeping in mind the electrode potential, which one of the following reactions is feasible?
Correct answer: C. Fe + CuSO4 → FeSO4 + Cu
- A. Zn+2 + Cu → Cu+2 + Zn
- B. Zn + MgSO4 → ZnSO4 + Mg
- C. Fe + CuSO4 → FeSO4 + Cu
- D. Cd + MgSO4 → CdSO4 + Mg
Explanation
Fe + CuSO₄ → FeSO₄ + Cu is feasible because iron has a lower reduction potential (-0.44 V) than copper (+0.34 V), meaning iron is more reactive and can displace copper from its salt solution. The positive cell potential (+0.78 V) confirms the reaction is spontaneous.
This question appeared on the UHS MDCAT 2015 paper, which you can sit online with every answer explained.
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About Redox Reactions
Redox reactions involve oxidation and reduction occurring together, with electrons transferred between species or oxidation numbers changing. The topic covers assigning oxidation states, identifying oxidizing and reducing agents, balancing redox equations by oxidation number or half-reaction methods, and connecting chemical changes with galvanic and electrolytic cells.
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