Consider the reaction: 2 NO(g) + 2H₂(g) → N₂(g) + 2 H₂O(g) Initial concentrations and rates for this reaction are given in the table below.

(a) From the data given, determine the order for each of the reactants, NO and H₂, show your reasoning, and write the overall rate law for the reaction.

(b) Calculate the value of the rate constant, k, for the reaction. Include units.

(c) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H₂ has been consumed.

(d) The following sequence of elementary steps is a proposed mechanism for the reaction.

Based on the data present, explain why the first step cannot be the rate determining step.

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Experiment 1 1234 2 4 Initial concentration (mol/L) [NO] 0.0060 0.0060 0.0010 0.0020 [H₂] 0.0010 0.0020 0.0060 0.0060 Initial rate of formation of N₂ (mol/L min) 1.8 X 10+ 3.6 x 10-4 0.30 x 104 1.2 x 104