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17 Nov 2019
The following mechanism has been proposed for the reaction of NO with H_2, forming N_2O and H_2O. Step 1: 2NO(g) rightarrow N_2O_2 (g) Step 2: N_2O(g) + H_2 rightarrow N_2O(g) + H_2O(g) Write the equation of the overall reaction for which this reaction is valid. Identify all intermediates in the mechanism. Determine the molecularity of each elementary step in the mechanism. Write the differential rate laws for the forward reactions of each elementary step in the mechanism. The observed rate law for the overall reaction is Rate = k[NO]^2. Which of the elementary steps is the rate-determining step? Explain.
The following mechanism has been proposed for the reaction of NO with H_2, forming N_2O and H_2O. Step 1: 2NO(g) rightarrow N_2O_2 (g) Step 2: N_2O(g) + H_2 rightarrow N_2O(g) + H_2O(g) Write the equation of the overall reaction for which this reaction is valid. Identify all intermediates in the mechanism. Determine the molecularity of each elementary step in the mechanism. Write the differential rate laws for the forward reactions of each elementary step in the mechanism. The observed rate law for the overall reaction is Rate = k[NO]^2. Which of the elementary steps is the rate-determining step? Explain.
Casey DurganLv2
29 Jan 2019