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

And if we start with a #0.025*mol# quantityof permanganate, what quantity of peroxide is required?

Answer 1

You gots......

#2MnO_4^(-)+6H^+ + 5H_2O_2 rarr 2Mn^(2+) + 5O_2 + 8H_2O#

This means that the equation is now stoichiometrically balanced in terms of mass and charge, which is a necessary condition for a chemical equation to be a true representation of reality.

Do you agree that five equiv hydrogen peroxide are oxidized by two equiv permanganate?

We start with #0.025*mol# permanganate...and thus we need....

#0.025*molxx5/2=0.0625*mol# 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 #Mn^(2+)# ion.

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Answer 2

Avery Adams

[ 2 \text{KMnO}_4 + 5 \text{H}_2\text{O}_2 + 3\text{H}_2\text{SO}_4 \rightarrow 2\text{MnSO}_4 + 5\text{O}_2 + 8\text{H}_2\text{O} + K_2\text{SO}_4 ]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.