A solution of cuso4 was kept in an iron pot. After few days, the iron pot was found to have a number of holes in it. Write the equations of the reaction that took place. Explain this reaction in terms of reactivity of metals.
Answers
Explanation:
Metals and Non-metals. A solution of copper sulphate was kept in an iron pot. ... Iron is more reactive than copper and so iron displaces copper from copper sulphate solution. Since iron is being consumed, holes appear in the pot.
Answer:
Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactants change. Redox is a reduced form of reduction-oxidation. 2 different processes—a reduction process and an oxidation process—can be used to describe all redox reactions.
Explanation:
Iron displaces copper because it is more reactive than copper and produces FeSO₄ as a result. During this procedure, some of the iron dissolves, leaving holes in the pot.
Fe (iron) + CuSO₄ (copper sulfate) → FeSO₄ (iron sulfate) + Cu (copper)
The following two steps occur in this reaction:
1. Reduction process; Cu²⁺ is the oxidizing agent.
Cu²⁺ + 2e⁻ → Cu0
2. In the oxidation process, when Fe(0) serves as the reducing agent,
Fe(0) - 2e⁻ → Fe²⁺
The process might be a redox reaction or a two-fold displacement reaction (oxidation and reduction both take place simultaneously).
Hence, the required equation is CuSO₄ + Fe → FeSO₄ + Cu
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