Conduct the Following in complete sentences and/or diagrams and/or The mechanism for the autoxidation of hydrocarbons...
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...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.) 12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
The reaction between nitric oxide (nitrogen monoxide) and oxygen gives nitrogen dioxide according to the stoichiometric equation. 2 NO(g) 02(g)2 NO2(g) 1. Write the rate law expected if the reaction was found to occur in a single step The reaction is observed to be complex with the following mechanism is proposed: 2 NO N202 N202 2 NO N202 +02 → 2NO2 k2 kı k. -1 2. Use the steady state approximation to obtain the expression for the formation of NO2....
What is the rate law derived from the following mechanism? Step 1: 2 NO (g) = N2O2 (g) (fast) Step 2: N2O2 (g) + O2 (g) —+2 NO2 (g) (slow) Rate = k[NO]2[02] Rate = k[N202][02] Rate = k[N202] Rate = k[NO]2
3. According to the mechanism 2NO ki ki N202 N202 + 02 -k2 → 2NO2 Under steady state approximation, what is the rate of formation, (v), of nitrogen dioxide, NO2, when the oxygen concentration is very low?
i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O + H30+ +02 (a) The intermediate in the proposed mechanism is The catalyst is (b) Apply the steady state approximation to this mechanism to deduce the rate law in terms of d[O2]/dt. (15 pts)
What is the rate law for overall reaction? Consider the following mechanism: Step 1: 03 → 02 + 0 Step 2: 03 + 0 + 2O2 (fast) (slow)
What is the rate law derived from the following mechanism? Step 1: 2 NO(g) N2O2(g) (fast) Step 2: N2O2(g) + O2(g) —>2 NO2 (g) (slow) Rate = k[NO]2 Rate = k[NO]2[02] Rate = K[N2021 Rate = K[N202][02]
Ozone decomposes to molecular oxygen: 2 O3(g) ⇋ 3 O2(g). The following is a proposed mechanism for the reaction: Step 1: O3(g) ⇋ O2(g) + O(g) (fast) Step 2: O3(g) + O(g) ⇋ 2 O2(g) (slow) Provide a valid rate law for the overall ozone decomposition reaction based on this mechanism. 4. Ozone decomposes to molecular oxygen: 203(g) — 3 O2(g). The following is a proposed mechanism for the reaction: Step 1: 03(g) – O2(g) + O(g) (fast) Step 2:...
The reaction 2A + B → C occurs by the following 2 step mechanism: A + B ------(k1)------> AB AB ------(-k1) ------> A+B AB + A ----- (k2)------> C Apply the steady-state approximation for the reaction intermediate concentration to obtain the overall rate law from this mechanism: a) k1 [A][B] b) k1k2[A][B]/((-k1) - k2[A]) c) k1k2[A]^2[B]/((-k1)+k2[A])