this is all one question

Experiments were conducted to study the rate of the reaction represented by this equation. 2H2(3) + 2NO(g) - N2(g) + 2H20 (3) Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data: Experiment Initial Concentration Initial Concentration Initial Rate of Formation of [NO] (mol/L) [H2] (mol/L) N2 (W/min) 1 0.0060 0.0010 1.8 x 10-4 2 0.0060 0.0020 3.6 x 10-4 3 0.0010 0.0060 0.30 x 10-4 4 0.0020 0.0060 1.2 x 10-4 Consider the following questions: (a) Determine the order for each of the reactants, NO and Hz, from the data given. NO Ozero order O first order second order O third order H zero order O first order O second order third order (b) Write the overall rate law for the reaction. Rates (c) Calculate the value of the rate constant, k, for the reaction. Include units. unit: (d) For experiment 2. calculate the concentration of NO remaining when exactly one half of the original amount of He had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO + NO + N20 Step 2: N2O + H2 + H2O + N20 Step 3: N2O + H, N, + H2O Based on the data presented, which of these is the rate determining (slow) step? Submit