# What is the stoichiometric equation for the oxidation of hydrogen peroxide by potassium permanganate?

## And if we start with a $0.025 \cdot m o l$ quantityof permanganate, what quantity of peroxide is required?

Sep 13, 2017

You gots......

$2 M n {O}_{4}^{-} + 6 {H}^{+} + 5 {H}_{2} {O}_{2} \rightarrow 2 M {n}^{2 +} + 5 {O}_{2} + 8 {H}_{2} O$

#### Explanation:

Now the equation is stoichiometrically balanced with respect to mass and charge. And this is an absolute requirement for a chemical equation, a representation of reality.

Two equiv permanganate oxidize five equiv hydrogen peroxide. Do you agree?

We start with $0.025 \cdot m o l$ permanganate...and thus we need....

$0.025 \cdot m o l \times \frac{5}{2} = 0.0625 \cdot m o l$ with respect to peroxide.....

What would you see in the reaction? Well evolution of gas for one, and second, the deep red colour of permanganate would dissipate to give effectively COLOURLESS $M {n}^{2 +}$ ion.