Redox reactions refer to a pair of reactions in which a particular oxidation is coupled to a corresponding reduction. Although neither can occur independently of the other, it can be helpful to write each oxidation or reduction as a half reaction to help us understand and calculate the flow of energy. In this exercise, sort each listed half reaction as either an oxidation or a reduction.

The Equations sort each listed half reaction as either an oxidation or a reduction.

Fe + CuSO4 + → FeSO4 + Cu

(Fe oxidized, Cu reduced)

Explanation:

For proper understanding of the concept of the Redox reaction, let us know the meaning:

Reduction- Oxidation or "redox" reactions occur when elements in a chemical reaction gain or lose electrons. This reaction causes an increase or decrease in oxidation numbers. The Half Equation Method is used to balance these reactions. The equation is separated into two half-equations, one for oxidation and one for reduction. For Example -

CuO + H2 → Cu +H2O.

In this redox reaction, CuO is getting reduced to Cu since Oxygen is getting removed.

Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) Oxidation state of Fe changes from 0 to +2 and oxidation state of Cu changes from +2 to 0.

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