Question

Using the chemical equation, determine how to determine the amount of H2O2 from a reaction that required 7.84 mL of 0.15 M KMnO4.

5H₂O₂+ 2KMnO₄+ 3H₂SO₄à K₂SO₄+ 2MnSO₄+ 8H₂O + 5O₂

Answer 1

Given equation-

5H2O2 + 2KMnO4 + 3H2SO4 →K2SO4 + 2MnSO4 + 8H2O + 5O2

Moles of KMnO4 required= molarity*volume= 0.15 M *7.84ml=0.15mol/L*7.84 *10^-3 L=0.001176 moles

From equation you can figure out that, 2 moles KMnO4 reacts with 5 moles H2O2

So 1 mol KMnO4 reacts with 5/2=2.5 moles H2O2

Hence, 0.001176 moles of KMnO4 reacts with 2.5*0.001176 (=0.00294) moles H2O2

Answer= Amount of H2O2=0.00294 moles