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 in the rate law expression.
3. A proposed mechanism for the decomposition of ozone, O3, is as follows:
Step 1 O3 -->/<-- O2 + O fast
Step 2 O3 + O --> 2O2 slow
a. What is the overall reaction?
b. Identify the intermediates in the reaction mechanism.
c. Write a rate law expression for each step including any reversible reactions.
d. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.
4. Consider the following 3 step reaction mechanism:
Step 1 H2 --->/<-- 2H fast
Step 2 H + CO --> HCO slow
Step 3 H + HCO --> H2CO fast
a. What is the overall reaction?
b. Identify the intermediates in the reaction mechanism.
c. Write a 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 in the rate law expression.
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
#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...
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...
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....
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow N O 2 ( g ) + C l 2 ( g ) → C l N O 2 ( g ) + C l ( g ) S l o w NO2(g)+Cl(g)→ClNO2(g)Fast a)What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. b)Identify the intermediates in the mechanism. Check all that apply. Check all that apply. NO2(g), ClNO2(g), Cl2(g) ,Cl(g)...
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.
The reaction 2 NO2 --> 2 N2 + O2 follows the mechanism: Step 1: NO2 --NO NO3 NO2 SLOW + + Step 2: NO3 CO FAST NO2 CO2 -> + What is the intermediate in the reaction? none of these NO2 ONO3 OOOO
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...
2NO2 +Cl2 ----> 2NO2Cl mechanism: NO2 +Cl2 -----> NO2Cl +Cl (Slow step) NO2 +Cl -----> NO2Cl (fast step) using the mechanism, draw and energy profile of the reaction showing the relative energy of the reactants and products (this reaction is exothermic), both transition states, intermediates, activation energy for both steps, and the overall change in enthalpy for the reaction (Delta H of the reaction).
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2] 2. What is the overall reaction? A. 2 NO2 + F2 → 2 NO2F B. NO2 + F2 → NO2F +F + NO2 C. NO2 + F2 → 2 NO2F 3. Write out...
3a. Write the overall reaction equation for the following mechanism. Identify the intermediates. fast slow fast 02 20 O+N2 NO N b. The rate law for the following mechanism is rate kIN2] [O]. Show how this can be determined from the mechanism. c. Draw a possible energy diagram for this reaction and show the location of the reactants, products, and intermediates. Reaction progress