1) Decomposition of Ozone Upon interaction with UV radiation, ozone decomposes into oxygen, a process described...
1)
Decomposition of Ozone
Upon interaction with UV radiation, ozone decomposes into oxygen, a process described in the following overall
chemical reaction:
2O3(g)<-->3O2(g)
The elementary reactions of the decomposition of ozone are:
O3<--K1__K-1-->O2+O (fast)
O+O3 --k2--> 2O2 (slow)
(a) Why does it make sense that the first elementary reaction is fast compared to the second one?
(b) Write out the rate laws for the elementary reactions in part a.
(c) Based on your answers in part a, what is the rate law of the overall reaction? Make sure your rate law
does not contain concentrations of intermediates.
(d) You may (or may not) have found that one of your reagents has a negative order in the rate law for the
overall reaction. What would it mean for a reagent to have a negative order, in terms of how it affects the
overall reaction rate? (Hint: if you were performing an experiment to determine the rate law, how would
the rate be affected if you added more of the reagent with a negative reaction order?) Why would this be
the case?
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1)
Decomposition of Ozone
Upon interaction with UV radiation, ozone decomposes into
oxygen, a process described...
Ozone decomposes to molecular oxygen: 2 O3(g) ⇋ 3 O2(g). The following is a proposed mechanism...
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:...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
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...
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2  
#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...
Chapter 14 and 15 1) Ozone decomposes to oxygen gas. 20, (g) ---> 30, (9) A...
Chapter 14 and 15 1) Ozone decomposes to oxygen gas. 20, (g) ---> 30, (9) A proposed mechanism for this decomposition is o, =====> 0, +O (fast, equilibrium) O, + ---> 20% (slow) What is the rate law derived from this mechanism? 2) N2(g) + 3 H2(g) — > 2 NH3(g) Kc = 11.60 at 600 °C. Calculate Kp for this reaction at this temperature. 3) The rate of a particular reaction doubles when the temperature is increased from 250...
One of the components of smog is ozone,O3, a colorless, toxic gas. It is a very...
One of the components of smog is ozone,O3, a colorless, toxic gas. It is a very strong oxidizing agent and causes respiratory illnesses. Ozone is produced in the lower atmosphere due to the catalytic effect of nitric oxide, NO, a byproduct of the combustion process in car engines. However, in the upper atmosphere ozone is a very useful gas, because it absorbs ultraviolet radiation and protects the earth from this high energy, damaging radiation. It is referred to as the...
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction...
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...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have been proposed to account for this reaction. Mechanism 2 03 302 bimolecular, rate constant k Mechanism II 03 02 + fast equilibrium, equilibrium constant K1 0+ 03 — 202 slow, rate constant k2 A. Derive rate laws for the formation of O2 for each mechanism. B. Thermodynamic measurements give standard enthalpies of formation for each of the following species at 298 K: species AH°...
please 6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall...
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:...
Plot the natural log of the concentration of the ozone Versus time. Since we get a...
Plot the natural log of the concentration of the ozone Versus time. Since we get a straight line, that mean., that we can consider an integrated rate law for this reaction to be given by the following: ln([O_3]/[O_3]_o) = -kt How long does it take for half the ozone to decompose, and what is the concentration of ozone at that time? What is the initial reaction rate of the ozone decomposition reaction? Provide both the magnitude and the units. What...
13 Interpreting Mechanisms S20(1) - Protected View - Saved - Search References Mailings Review View ain...
13 Interpreting Mechanisms S20(1) - Protected View - Saved - Search References Mailings Review View ain viruses. Unless you need to edit, it's safe stay in Prolus i ew. Enable Editing Student Name: #13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Brz Step 2 Br + H2 Step 3 H2Br Br - fast 2Br H2Br 2HBO fast slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate...
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:...
Chapter 14 and 15 1) Ozone decomposes to oxygen gas. 20, (g) ---> 30, (9) A proposed mechanism for this decomposition is o, =====> 0, +O (fast, equilibrium) O, + ---> 20% (slow) What is the rate law derived from this mechanism? 2) N2(g) + 3 H2(g) — > 2 NH3(g) Kc = 11.60 at 600 °C. Calculate Kp for this reaction at this temperature. 3) The rate of a particular reaction doubles when the temperature is increased from 250...
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...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have been proposed to account for this reaction. Mechanism 2 03 302 bimolecular, rate constant k Mechanism II 03 02 + fast equilibrium, equilibrium constant K1 0+ 03 — 202 slow, rate constant k2 A. Derive rate laws for the formation of O2 for each mechanism. B. Thermodynamic measurements give standard enthalpies of formation for each of the following species at 298 K: species AH°...
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:...
Plot the natural log of the concentration of the ozone Versus time. Since we get a straight line, that mean., that we can consider an integrated rate law for this reaction to be given by the following: ln([O_3]/[O_3]_o) = -kt How long does it take for half the ozone to decompose, and what is the concentration of ozone at that time? What is the initial reaction rate of the ozone decomposition reaction? Provide both the magnitude and the units. What...
13 Interpreting Mechanisms S20(1) - Protected View - Saved - Search References Mailings Review View ain viruses. Unless you need to edit, it's safe stay in Prolus i ew. Enable Editing Student Name: #13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Brz Step 2 Br + H2 Step 3 H2Br Br - fast 2Br H2Br 2HBO fast slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate...
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