When a pink aqueous solution of potassium permanganate, faintlyacidified with dilute sulfuric acid was treated with 10% aq.hydrogen peroxide, the reaction took place with the evolution ofgas bubbles, and the pink solution was turned colorless. Furtherchemical analysis revealed that the evolved gas was oxygen, and theresulting solution contains potassium sulfate and manganese (II)sulfate; water was also formed during the same reaction. Pleaseanswer the followings: 1) Write down the proper chemical equationfor this reaction. 2) Balance the chemical equation. 3) Define thetype/types of the reaction, and offer an explanation for the colorchange. 4) Write down the ions (and define types) present in thesolution before & after the reaction. 5) If initially 5.65 g ofpotassium permanganate was taken for the reaction, calculate thetotal number of moles of manganese (II) sulfate present in thesolution after the completion of the reaction
