(Solved): help is appreciated! In a study of the gas phase decomposition of hydrogen peroxide at \( 400^{\circ ...

In a study of the gas phase decomposition of hydrogen peroxide at \( 400^{\circ} \mathrm{C} \) \[ \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{V} / 2 \mathrm{O}_{2}(9) \] the concentration of \( \mathrm{H}_{2} \mathrm{O}_{2} \) was followed as a function of time. It was found that a graph of \( 1 /\left[\mathrm{H}_{2} \mathrm{O}_{2}\right] \) versus time in seconds gave a straight line with a slope of \( 0.988 \mathrm{M}^{-1} \mathrm{~s}^{-1} \) and a y.intercept of \( 4.42 \mathrm{M}^{-1} \). Based on this plot, the reaction is order in \( \mathrm{H}_{2} \mathrm{O}_{2} \) and the rate constant for the reaction is