# Question 3e7df

Jan 20, 2017

$2 \stackrel{+ 2}{H} g {\left(\stackrel{+ 5}{N} {\stackrel{- 2}{O}}_{3}\right)}_{2} \stackrel{\Delta}{\to} 2 \stackrel{0}{H} g + 2 \stackrel{+ 4}{N} {O}_{2} + {\stackrel{0}{O}}_{2}$

The changes in oxidation number of elements in the given reaction are as follows

$\stackrel{+ 2}{H} g \to \stackrel{0}{H} g \implies \text{2 unit reduction}$

stackrel(+5)N->stackrel(+4)N=>"1 unit reduction"#

$\stackrel{- 2}{O} \to \stackrel{0}{O} \implies \text{2 unit oxidation}$

It is obvious from above change in ON that the reaction is an intramolecular redox reaction brought about by heat.

Jan 22, 2017

Noting that one reactant is producing several simpler products I would just call it a (thermal) decomposition.