rate depends on the slowest step
Here 2nd step is slowest
So, rate law is:
rate = k2[O3][O]
We need to remove intermediate which is O
we will use 1st step:
Kc = [O2][O]/[O3]
[O] = Kc[O3][O2]-1
put this in rate law expression above:
rate = k2[O3][O]
rate = k2[O3]Kc[O3][O2]-1
let k2Kc be k
so,
rate law becomes:
rate = k[O3]2[O2]-1
Hence proved
5. Ozone in the atmosphere decomposes by the following reaction: The experimentally observed rate law is...
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:...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O:(g) + O(g) →202(g): rate = k[O][NOJ Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H2O2(aq) + I'(aq) → H2O(l) + Of(aq) ---...-slow H2O2(aq) + Or(aq) → H2O(0) + O2(g) + I'(aq) -----fast What...
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: rate k[O][NO] Os(g)+O(g)+20;(g); Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: -slow H2O:(aq) +I(aq)H;O(1) + 0I°(aq) -fast H20:(aq) +Or(aq)H:O()) +02(g)+l'(aq) What is: iv) the catalyst? iv) the intermediate ii) the rate law i) the...
A proposed mechanism for one of the pathways for the destruction of ozone in the atmosphere is: step 1 slow: O3 + NO ---->NO2 + O2 step 2 fast: NO2 + O -----> NO + O2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. _____+_____----->_____ (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank:(2) Which species acts as...
The following mechanism has been proposed for the conversion of ozone to oxygen in the gas phase. step 1 fast: O3O step 2 slow: 03 + 0-202 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is...
3. Propose a mechanism and rate-limiting step that are consistent with the experimentally observed rate law. (20 pts) kKAPA A → B+C (1 + PAKA + Pg KB + PcKc)2
Please answer each part with work shown. Thank you.
6. The following three mechanisms have been proposed for a particular reaction. Mechanism II Mechanism III Mechanisml H2 +NO-H2O+N (slow) N +NON2+0 (fast) O+H2-> H2O (fast) 2 NO-N202 (fast equilibrium) H2-N202-H20+ N3O (slow) H2+N20-H2O+N2 (fast) H2 + 2 NO- H2O+N2O (slow) N20+ H2N2+ H2O (fast) a) What is the overall reaction that each proposed mechanism supports? b) Calculate the ΔΗ'm for the overall reaction. c) For each mechanism, draw an energy...
please
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O(g) + O(g) 20(8): rate-k[O][NO] Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H:Os(aq) + (aq) → H2O(1) Ol(aq) --- -slow H2O2(aq) + Ol'(aq) → H2O(1) + O2(g) + l'(aq) ------fast What is:...
Consider the overall reaction.... A+B--C+D which has an observed rate law of Rate=k[A12 Which of the following choices would be a sensible 2-step mechanism, given this observed rate law? O A+A-->E slow E+B-->C+D fast A+B--> 2 E --> C+D fast slow A+A-->E E+B-->C+D fast slow A+B-->E 2 E -->C+D slow fast
4. The following mechanism has been suggested for the decomposition of ozone, Os. 0:(9) 02(g) +O(g) (fast equilibrium) O(g) + O2(g) → 20 (9) (slow) Consider the following statements in light of this mechanism: 1. The rate law is second order in O. 2. The rate does not depend on the concentration of Oz 3. The reaction slows with increased O, concentration 4. The rate law is second order 5. substances reacting with O atoms will speed up the reaction...