3—Part II: For the following hypothetical mechanism Step (1) slow 2 A+ E + C +...
4. Below is a proposed mechanism for a reaction: Step 1. Step 2. C+E-F Step 3. F G A B C+D Fast equilibrium Slow Fast A. (2 points) What is the overall stoichiometry for this reaction? B. (2 points) Which step is the rate determining step? C. (6 points) If this mechanism is correct, what should the rate equation for this reaction be? (Make sure you include the fast equilibrium)
Consider the mechanism. Step 1: AB+C Step 2: C+ DE Overall: A+D- B+E slow fast Determine the rate law for the overall reaction, where the overall rate constant is represented ask. rate =
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...
Consider the following mechanism. Step 1: A+B → C slow step 2: A+C→ D fast overall: 2A+B → D Determine the rate law for the overall reaction (where the overall rate constant is represented as k). rate w
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...
Consider the mechanism. 2A - B slow Step 1: Step 2: Overall: B + C -→ D fast 2 A + C -- D Determine the rate law for the overall reaction, where the overall rate constant is represented as k.
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C (slow) 1. What is the overall reaction? [Select] 2. What is the intermediate in the mechanism? (Select] 3. What is the molecularity of step 1? (Select 4. Which step is the rate determining step? [Select) 5. What is the rate law predicted by this mechanism? [Select) Question 22 15 pts Consider the following reaction at equilibrium: CO(g) + 2H2(g) CH2OH(g) AH=-18 kJ How will...
Name Wkst #16 CHEM& 162 1. Consider the following proposed reaction mechanism. 12 = 21 1 + O₂ → 10₂ + 0 0+ 03 - 202 1 +10, -12 + O2 A. What is the overall reaction? B. What are the intermediates and catalysts? Intermediates: Catalysts: C. If the first step is in equilibrium and the second step is slow. what is the overall rate law? Remember, intermediates cannot appear in the final rate law! Rate = D. On the...
11. Below are 2 possible reaction mechanisms (pathways) for the reaction Mechanism 1 No, + 03 → No, (fast) NOs + NOs → N20s + 5/202 (slow) Mechanism 2 NO2 + 03 → NO3 + 02 (slow) No, + NO2 → N20s (fast) If the reaction rate law is found to be: rate = k[NO21 Which mechanism is consistent with this rate law (1 or 2) What is/are the intermediate/s for Mechanism 1? What is/are the intermediate/s for Mechanism 2?...
Consider the three-step mechanism for the reaction of A through intermediates B and C to produce D shown below. A → B Ea = 6 kcal/mol, ΔH° = 4 kcal/mol B → C Ea = 4 kcal/mol, ΔH° = -10 kcal/mol C → D Ea = 13 kcal/mol, ΔH° = -6 kcal/mol A. draw and label and energy diagram. B. what is the overall enthalpy?