# How do you convert N_2 to NH_3 and NO_3^-?

Mar 3, 2017

$\text{By oxidation to nitrate, or by reduction to ammonia..............}$

#### Explanation:

$\text{Reduction:}$

$\frac{1}{2} {N}_{2} + 3 {H}^{+} + 3 {e}^{-} \rightarrow N {H}_{3}$

$\text{Oxidation:}$

$\frac{1}{2} {N}_{2} + 3 {H}_{2} O + \rightarrow N {O}_{3}^{-} + 6 {H}^{+} + 5 {e}^{-}$

Charge and mass are balanced (I think) in each reaction, as indeed they must be if these are viable representations of chemical reactivity,

Both reactions are viable, and need some form of reducing or oxidizing agent.