Consider the following mechanism:
O3 => O2 + O
NO + O => NO2
What is the role of O
Consider the following mechanism: O3 => O2 + O NO + O => NO2 What is...
What is the role of NO(g) in the reaction mechanism below? NO(g) + O3(g) --> NO2(g) + O2(g) O(g) + NO2(g) --> NO(g) + O2(g)
The proposed mechanism for a reaction is O3 => O2 + O Slow O + NO => NO2 Fast Which of the following would be a rate law for the reaction?
Consider the reaction of NO2 with ozone O3 to produces NO3 and O2. What factor(s) will affect the rate of this reaction ? A. [NO2] and [O3] B. [NO3] and [O2] C. temperature D. [NO2] and [O3] and temperature of the reaction E. [NO3] and [O2] and temperature of the reaction
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...
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.
NO + O3 --------> NO2* + O2 If NO2* chemiluminescence is centered at 1200 nm, what should be the minimum ΔG for the above reaction? If the reaction is endothermic, will it still be able to chemiluminesce?
1. Consider the following thermochemical equation. NO (g) +O3 (g) → NO2 (g) + O2(g) ΔΗ--1 99 kJ a) This reaction is i. endothermic ii. exothermic b) Calculate the amount of energy (kJ) released when 8.50 g of NO (g) is reacted with an excess of ozone, O3
What is O3, O2, and O Step1: Cl + O3 ⇄ ClO + O2 Step2: ClO + O ⇄ Cl + O2 Total: O3 + O ⇄ 2O2 a. Cl(catalyst) b. O3 c. ClO(intermediate) d. O2 e. O
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 rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...