Hydrogen peroxide, $H_2{O}_{2(aa)},$ must be stored at low temperatures to reduce the rate at which it decomposes to water and oxygen. The decomposition reaction is shown in the equation below.

$2H_2{O}_{2(xa)}2H_2{O}_{(1)}+O_{2(3)}$

A student wants to investigate the rate of decomposition of $H_2{O}_{2(aq)}$ at room temperature and pressure. They set up an experiment that will measure the volume of oxygen gas produced over time. The student uses $30\mathrm{.}0c{m}^3$ of $2\mathrm{.}50mold{m}^{-3}{H}_2{O}_2.$ The student collects results at a series of time intervals and uses that data collected to determine the concentration of $H_2{O}_{2(\text{m}\text{a}\text{q})}$ at each time. They then use this data to plot a concentration$-$time graph as shown in figure $4.$

Figure $4$: Concentration$-$time graph for the decomposition of hydrogen peroxide

Determine the number of moles of oxygen that have been produced throughout the duration of the experiment.