# Can you represent the reduction of perchlorate to chloride by oxidation of NO_2 to nitrate anion?

May 26, 2017

Well, $\text{perchlorate ion}$ is reduced from $C l \left(V I I +\right)$ to $C l \left(- I\right)$....

#### Explanation:

$C l {O}_{4}^{-} + 8 {H}^{+} + 8 {e}^{-} \rightarrow C {l}^{-} + 4 {H}_{2} O \left(l\right)$ $\left(i\right)$

And $N {O}_{2}$ is oxidized, $N \left(I V +\right)$ to $N \left(V +\right)$:

$N {O}_{2} \left(g\right) + {H}_{2} O \rightarrow N {O}_{3}^{-} + 2 {H}^{+} + {e}^{-}$ $\left(i i\right)$

And so to eliminate the electrons, we take $\left(i\right) + 8 \times \left(i i\right)$:

$8 N {O}_{2} \left(g\right) + 4 {H}_{2} O + C l {O}_{4}^{-} \rightarrow 8 N {O}_{3}^{-} + 8 {H}^{+} + C {l}^{-}$

Is this balanced with respect to mass and charge?