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Reaction of permanganate with hydrogen peroxide: usefull information

Here, by following the above sequence of steps, the electron balance is very simply balanced and thus the laws of conservation of charge and conservation of mass are satisfied - take my online class for me . Permanganate ions oxidise hydrogen peroxide to oxygen in acidic solution and are themselves reduced to Mn2+.

Set up the partial equations for oxidation and reduction: main theory

Partial equation of reduction

First determine the oxidation numbers of the corresponding redox pairs - chemistry solver . Manganese in the permanganate ion has the oxidation number VII and as Mn2+ ion the oxidation number II. Permanganate therefore accepts 5 electrons:

Mn+VIIO4--II + 5 e - → Mn2++II

However, the charge and mass balance of the partial equation are not correct. The sum of the charges is -6 on the left and +2 on the right. Moreover, the oxygen atoms must appear on the product side.

Charge balance - do my assignment : The reaction takes place in the acidic, so the charge can be balanced by H+ ions. In the basic one, hydroxide ions, OH-, would be used.

MnO4- + 5 e- + 8 H+⇌ Mn2+.  

Now the sum of the charges on the left and right sides of the equation match (+2 each), but the oxygen atoms are still missing on the right side.

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