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 answer is
What is the role of NO(g) in the reaction mechanism below? NO(g) + O3(g) --> NO2(g)...
Consider the following mechanism: O3 => O2 + O NO + O => NO2 What is the role of O
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...
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
What is the G°rxn for the reaction in question? NO(g) + O(g) -> NO2(g) Grxn= -676.0kJ 2O3(g) -> 3O2(g) Grxn= +489.6kJ O2(g) -> 2O(g) Grxn = ?? NO(g) + O3(g) -> NO2(g) + O2(g) Grxn=-199.5kJ
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:...
Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (9) NO (g) + O2 (g) PE "IM Reaction path What is the overall rate law? Rate = k[O3] Rate = k[O3][0] Rate = k[O3][NO]
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. b. Determine the temperature(oC) at which the reaction is at equilibrium.
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....
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. Blank 1 b. Determine the temperature(oC) at which the reaction is at equilibrium.