Oxygen can be prepared by the reaction of potassium manganate(VII), $$\(\mathrm{KMnO}_{4}\)$$, hydrogen peroxide, $$\(\mathrm{H}_{2} \mathrm{O}_{2}\)$$, and sulfuric acid, $$\(\mathrm{H}_{2} \mathrm{SO}_{4}\)$$. Each $$\(\mathrm{H}_{2} \mathrm{O}_{2}\)$$ molecule loses two electrons in this reaction. The other products of the reaction are potassium sulfate, manganese(II) sulfate and water. How many moles of oxygen gas are produced when 1.0 mol of $$\(\mathrm{KMnO}_{4}\)$$ reacts with an excess of

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