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Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + )...
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + ) --> NO2 (g) rate = k2 suppose that k1<<k2, That is the first step is much slower than the second. Write the balanced chem equation for the overall chemical rxn Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k() Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant...
Another method for the destruction of ozone in the upper atmosphere is: Step 1: 03 (g)...
Another method for the destruction of ozone in the upper atmosphere is: Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (g) = NO (g) + O2 (g) PE "M Reaction path What will be the effect on the value of the equilibrium constant (K) if the concentrations of all reactants are doubled and the temperature remains the same? O the equilibrium constant (K) will quadruple O the equilibrium constant...
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...
For the overall reaction below, which of the following is the correctly written rate law? Overall...
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide...
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide (commonly called nitric oxide), NO, from high-flying jet aircraft. O3(g) + NO(g) → NO2(g) + O2(g) The rate expression is rate = k[O3][NO]. Which of the following mechanisms are consistent with the observed rate expression? (a) NO + 03 - NO3 + 0 (slow) NO3 +0 - NO2 + O2 (fast) O3 + NO → NO2 + O2 overall (b) NO + O3 ->...
why is the answer B? please give detailed/step by step explanation, please. thanks d) (1 mark)...
why
is the answer B? please give detailed/step by step explanation,
please. thanks
d) (1 mark) SO2(g) also reacts with O3(g) to produce SO3(g). (Reaction B) The reaction coordinate diagram is shown to the right. What is the rate law for this process? E, SO (ad) +O(g) SO(g) SO(g) + O(g) Reaction B. SO2(g) + 03(g) SO3(g) + O2(g) Rate k [SO2(9)1 C) Rate kISO(ad)Os(g) B) Rate a D) Rate k (s02(9) k [SO3(g)IO2(g)] 2. (9 mark)SO2(g) to SO3(g) conversion...
NUMBER 3 AND 4 PLEASE! I JUST NEED #3 AND 4 Ozone Formation: NO2(g), is formed...
NUMBER 3 AND 4 PLEASE! I JUST NEED #3 AND 4
Ozone Formation: NO2(g), is formed by chemical reactions involving N2(g) and O2(g) at the high temperatures Inside internal combustion engines in our cars. In the presence of sunlight, NO2(g) reacts with O2(g) to generate Os(s) as described by the following overall reaction: NO2(g) + O2(g) = NO(g) + O2(g) E = 306.5 l/mol This chemical process occurs in two steps, as illustrated in the potential energy diagram. In the...
from rxn mechanism 03+ no2 ->no3 +o2 (slow) no3+no2->n2o5 (fast) rate=k [o3]1 [no2]1 so here, I...
from rxn mechanism 03+ no2 ->no3 +o2 (slow) no3+no2->n2o5 (fast) rate=k [o3]1 [no2]1 so here, I see that order is 1 for [o3] and [no2] because o3 + no2 has 1 coefficient in front. but my question is I learned that the order of reaction is not equal to the coefficient of species. !! so why coefficient is determined when writing rate of reaction here? this does not make sense to me.
Another method for the destruction of ozone in the upper atmosphere is: Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (g) = NO (g) + O2 (g) PE "M Reaction path What will be the effect on the value of the equilibrium constant (K) if the concentrations of all reactants are doubled and the temperature remains the same? O the equilibrium constant (K) will quadruple O the equilibrium constant...
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:...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
57.) The ozone, O3, of the stratosphere can be decomposed by reac- tion with nitrogen oxide (commonly called nitric oxide), NO, from high-flying jet aircraft. O3(g) + NO(g) → NO2(g) + O2(g) The rate expression is rate = k[O3][NO]. Which of the following mechanisms are consistent with the observed rate expression? (a) NO + 03 - NO3 + 0 (slow) NO3 +0 - NO2 + O2 (fast) O3 + NO → NO2 + O2 overall (b) NO + O3 ->...
why
is the answer B? please give detailed/step by step explanation,
please. thanks
d) (1 mark) SO2(g) also reacts with O3(g) to produce SO3(g). (Reaction B) The reaction coordinate diagram is shown to the right. What is the rate law for this process? E, SO (ad) +O(g) SO(g) SO(g) + O(g) Reaction B. SO2(g) + 03(g) SO3(g) + O2(g) Rate k [SO2(9)1 C) Rate kISO(ad)Os(g) B) Rate a D) Rate k (s02(9) k [SO3(g)IO2(g)] 2. (9 mark)SO2(g) to SO3(g) conversion...
NUMBER 3 AND 4 PLEASE! I JUST NEED #3 AND 4
Ozone Formation: NO2(g), is formed by chemical reactions involving N2(g) and O2(g) at the high temperatures Inside internal combustion engines in our cars. In the presence of sunlight, NO2(g) reacts with O2(g) to generate Os(s) as described by the following overall reaction: NO2(g) + O2(g) = NO(g) + O2(g) E = 306.5 l/mol This chemical process occurs in two steps, as illustrated in the potential energy diagram. In the...
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