What is oxidized and reduced in the following reactions? What is the oxidation a

Question

What is oxidized and reduced in the following reactions? What is the oxidation agent and the reducing agent? Which one releases electrons and receives electrons? How many electrons are transported?
Fe + CuSO4 -> FeSO4 + Cu
C6H6O6 + 6O2 -> 6H20 + 6C02

Explanation / Answer

A reducing agent is oxidised in redox, and an oxidising agent is reduced. Fe goes from oxidation number 0 to +2. It has lost electrons, so it is oxidised. It is the reducing agent. Cu goes from ON. +2 to 0. It has gained electrons, so it is reduced. Cu2+ is the oxidising agent. 2Fe + 3CuSO4 --> Fe2(SO4)3 + 3Cu It depends on what they specify which Fe it is, Fe(II) is missing 2 electrons, where as Fe(III) is lacking 3 electrons, so their charges will be 2+ and 3+ respectively. Both forms of Fe(II) and Fe(III) are abundant, so they must specify which one is being used, if not specified, I would go with a mixture of products such as: Fe2(SO4)3 and FeSO4.

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