
Consider the mechanism. 0, +NO, NO, +0, NO, +NO, — NO fast 0, +2NO, — 0,+N,0...
The mechanism for the gas-phase reaction 2NO + Cl2 → 2NOCl is suggested to be: (1) NO + NO → N2O4 (slow) (2) N2O4 + Cl2 → 2NOCl (fast) Based on this mechanism, the rate law for the overall reaction is: Select one: a. Rate = k [NO] b. Rate = k [NO]2 c. Rate = k [NO2]2[Cl2] d. Rate = k [Cl2]
step by step
Rates of Non-elementary reactions Class Activity Consider the following mechanism: 2NO N202 k-1 NzOz + C12-2+2 NOCI a. What is the net reaction? b. Which of the above species is an intermediate? Why? c. Find the rate of the overall reaction using the steady-state approximation. d. Repeat part (c) using the rate-determining step method, assuming the first-step is fast and at equilibrium and the second step is slow. 2NO N,02 (ast,at equilibrium) k-1 N202 + Cl2-22 NOCI...
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
a possible mechanism for the overall reaction is found below:Br2(g)+2NO(g)--->2NOBr(g). step 1: (fast) NO(g)+Br2(g)-->&<---NOBr(g) determine the rate law based on this mechanism. step 2 (slow) NOBr2(g) + NO(g)-->2NOBr(g)
3a. Write the overall reaction equation for the following mechanism. Identify the intermediates. fast slow fast 02 20 O+N2 NO N b. The rate law for the following mechanism is rate kIN2] [O]. Show how this can be determined from the mechanism. c. Draw a possible energy diagram for this reaction and show the location of the reactants, products, and intermediates. Reaction progress
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
Consider the following mechanism. Step 1: A+B → C slow step 2: A+C→ D fast overall: 2A+B → D Determine the rate law for the overall reaction (where the overall rate constant is represented as k). rate w
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2