In aqueous solution, hydrogen peroxide, $\text{H}_2\text{O}_2$, decomposes to form water and oxygen when an appropriate catalyst is present. $50\,\text{cm}^3$ of a $0.50\,\text{mol dm}^{-3}$ hydrogen peroxide solution gave $120\,\text{cm}^3$ of oxygen in $2.0$ minutes. The gas volume was recorded at room conditions. Calculate the average rate at which hydrogen peroxide decomposed over this $2.0$ minute interval.
- A$0.000083\,\text{mol dm}^{-3}\text{s}^{-1}$
- B$0.0083\,\text{mol dm}^{-3}\text{s}^{-1}$
- C$0.017\,\text{mol dm}^{-3}\text{s}^{-1}$
- D$0.10\,\text{mol dm}^{-3}\text{s}^{-1}$