Nitrogen dioxide, NO2(g), is produced as a by-product of the combustion of fossil fuels ininternal combustion engines. At elevated temperatures NO2(g) decomposes according to theequation below.11. 2 \mathrm{NO}_{2}(g) \rightarrow 2

\mathrm{NO}(g)+\mathrm{O}_{2}(g) The concentration of a sample of NO2(g) is monitored as it decomposes and is recorded onthe graph directly below. The two graphs that follow it are derived from the original data. A.) What order is the following reaction? B.) Write the rate law for the decomposition of NO2(g). C.) Consider two possible mechanisms for the decomposition reaction. i.) Is the rate law described by the mechanism I shown below consistent with therate law you wrote in part (b)? Justify your answer. Step 1: NO2(g) + NO2(g) → NO(g) + NO3(g)slow Step 2: NO3(g) → NO(g) + O2(g)fast ii.) Is the rate law described by mechanism II shown below consistent with the rate law you wrote in part (b) ? Justify your answer. Step 1:NO2(g) + NO2(g)N„O4(g)fast equilibrium Step 2:N204(9) → 2 NO(g) + O2(g)slow