$53)$ Magnesium ribbon, Mg $($s$),$ will burn in the presence of oxygen gas, forming solid magnesium oxide, MgO $($s$).$ The balanced chemical equation for this reaction is $2$ Mg $($s$)+$ O$2($g$)->2$ MgO $($s$)$ A chemical technician carries out this reaction three times at the same temperature, and collects the date given below. From the given information, determine the rate law, the rate constant, and the overall reaction order. Run Initial $[$Mg$]($mol$/$L$)$ Initial $[$O$2]($mol$/$L$)$ Rate $($mol$/$L s$)10\mathrm{.}100\mathrm{.}102\mathrm{.}0$ x $10-320\mathrm{.}200\mathrm{.}104\mathrm{.}0$ x $10-330\mathrm{.}100\mathrm{.}208\mathrm{.}0$ x $10-3$