Oxygen may be generated when potassium manganate(VII), $\text{KMnO}_4$, reacts with hydrogen peroxide, $\text{H}_2\text{O}_2$, in the presence of sulfuric acid, $\text{H}_2\text{SO}_4$. In this reaction, each $\text{H}_2\text{O}_2$ molecule is oxidised by losing two electrons. The remaining products are potassium sulfate, manganese(II) sulfate and water. What number of moles of oxygen gas are formed when $1.0\,\text{mol}$ of $\text{KMnO}_4$ reacts with excess $\text{H}_2\text{O}_2$ under acidic conditions?
- A$2.0\,\text{mol}$
- B$2.5\,\text{mol}$
- C$4.5\,\text{mol}$
- D$5.0\,\text{mol}$