During the reaction of $\text{K}_2\text{MnO}_4$ with concentrated hydrochloric acid, chlorine molecules and $\text{MnCl}_2$ are formed. Every manganese atom is reduced to $\text{MnCl}_2$. The oxidation numbers of both Mn and Cl alter in the reaction. No other element is oxidised or reduced. From these oxidation number changes, how many moles of chlorine are produced when $1.0\,\text{mol}$ of $\text{K}_2\text{MnO}_4$ reacts with an excess of hydrochloric acid?
- A$2.0\,\text{mol}$
- B$2.5\,\text{mol}$
- C$3.0\,\text{mol}$
- D$4.0\,\text{mol}$