Balance the following equations by oxidation-reduction...

Balance the following equations by oxidation-reduction methods; note that three elements change oxidation state.
$\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(s) \longrightarrow \mathrm{Co}_{2} \mathrm{O}_{3}(s)+\mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$

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Key Concepts

Half-Reaction Method

The half-reaction method involves splitting a redox reaction into two separate parts: one for oxidation and one for reduction. Each half-reaction is balanced individually for mass and charge, and then combined to give the balanced overall reaction. This systematic approach is especially useful for complex redox reactions.

Conservation of Mass and Charge

In any chemical reaction, particularly redox reactions, the law of conservation of mass and charge must be upheld. This means that all atoms and electric charges are balanced on both sides of the equation; a principle which guides the systematic balancing of redox equations.

Redox Reactions

Redox reactions are processes in which electrons are transferred from one species to another. This electron transfer changes the oxidation states of the elements involved and is characterized by the occurrence of both oxidation (loss of electrons) and reduction (gain of electrons) within the reaction.

Oxidation States

Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate the degree of oxidation of an element. This concept is crucial for identifying which elements are oxidized and which are reduced in a reaction, serving as a guide for balancing redox reactions.

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