An aqueous solution of hydrogen peroxide is added to a flask and breaks down, as shown. $\text{2H}_2\text{O}_2(aq) \rightarrow \text{2H}_2\text{O}(l) + \text{O}_2(g)$ The total volume of oxygen gas released is $180\,\text{cm}^3$ after $90$ seconds, measured at room conditions. The rate of the reaction is found using the equation shown. $\text{rate} = \frac{\text{change in moles of } \text{H}_2\text{O}_2}{\text{time}}$ What is the mean rate of the reaction, in $\text{mol min}^{-1}$, during the experiment?
- A$8.33 \times 10^{-5}$
- B$1.67 \times 10^{-4}$
- C0.0050
- D0.010