#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 not intermediates in the rate law expression.
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.
I have solved it for part 1. Kindly do similarly for the rest of the questions. Arrows and rate constants are not provided in the question. If the reaction is in equillibrium or not, I am not able to make it out. I will be able to give full justice to the solution if you provide me the full data. Thank you.
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2  
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 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...
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)...
3. Use the proposed reaction mechanism to answer the following questions; Elementary 1: 2NO2Cl <---> ClO2 + N2O + ClO Elementary 2: N2O + ClO2 <---> NO2 + NOCl Elementary 3: NOCl + ClO ---> NO2 + Cl2 a) What is the overall (reduced) reaction? b) Identify any intermediates. c) Determine the rate law expression for each elementary reaction. (fast) (fast) (slow)
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
1. The following mechanism has been proposed for the pas-phase reaction of chloroform and chlorine Ch> 20 (fast) CI + CHCI, - HCI +CCI, (slow) Cl + CCI - CCI (fast) a) Identify any intermediate(s): b) Identify any catalyst(s): b) Write the balanced equation for the overall reaction: c) Molecularity of each step: step 1. step 2. step 3 d) rds (circle): 1 2 3 d) What is the observable rate law predicted by this mechanism? e) What is the...
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).
Please answer each part with work shown. Thank you. 6. The following three mechanisms have been proposed for a particular reaction. Mechanism II Mechanism III Mechanisml H2 +NO-H2O+N (slow) N +NON2+0 (fast) O+H2-> H2O (fast) 2 NO-N202 (fast equilibrium) H2-N202-H20+ N3O (slow) H2+N20-H2O+N2 (fast) H2 + 2 NO- H2O+N2O (slow) N20+ H2N2+ H2O (fast) a) What is the overall reaction that each proposed mechanism supports? b) Calculate the ΔΗ'm for the overall reaction. c) For each mechanism, draw an energy...
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step...