# How to solve this redox reaction?

## Ni3O4 + HCl => NiCl2 + H2O + Cl2 How to solve this redox reaction using partial reaction method?

Nov 26, 2017

Reduction involves gaining electrons from a species that was oxidized (e.g. lost electrons). We calculate these through oxidation states, which I've omitted for clarity.

We'll divide it into oxidation and reduction reactions, and balance each in turn, making sure to keep the electrons transferred constant, as well. Hence,

$N {i}_{3} {O}_{4} + H C l \to N i C {l}_{2} + {H}_{2} O + C {l}_{2}$

Will divide into,

$2 {H}^{+} + N {i}_{3} {O}_{4} + 6 H C l + 2 {e}^{-} \to 3 N i C {l}_{2} + 4 {H}_{2} O$

$2 H C l \to C {l}_{2} + 2 {H}^{+} + 2 {e}^{-}$

$2 H C l \to C {l}_{2} + 2 {H}^{+} + 2 {e}^{-}$
$2 {H}^{+} + N {i}_{3} {O}_{4} + 6 H C l + 2 {e}^{-} \to 3 N i C {l}_{2} + 4 {H}_{2} O$
$- - - - - - - - - - - - - - - - - -$
$8 H C l + N {i}_{3} {O}_{4} \to C {l}_{2} + 3 N i C {l}_{2} + 4 {H}_{2} O$