Help me with my study guide The reaction shown below is an isomerization from AF. The reaction has 4 intermediates (B, C, D, E).Answer the following questions regarding this reaction.H+-OHBHΘΗΙ-όπ+ H₂O+ H₂OE+H-F-OHa) Draw the energy diagram for this reaction assuming that the second step (B⇒C) is the rate determining stepand the overall reaction is exergonic. Label each axis.b) Draw the reactant, product or intermediate present at each point (A-F) in the diagramc) Why does the carbocation rearrange in the third step (e.g. C→D)?

a) Energy DiagramTo draw the energy diagram:Assume that B → C is the rate-determining step…

Answered: The reaction shown below is an…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter8: Addition Via Carbocation

Section: Chapter Questions

Problem 22CTQ

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In each of the following three reaction coordinate diagrams, state: (a) Whether the reaction is exothermic or endothermic. (b) Whether the reaction is the slowest, the fastest, or intermediate in rate. (c) If all three reactions have the same entropy change between the reactant and product, which reaction has the largest favorable G0.
9. Sketch an energy diagram for a one-step reaction that is fast and exergonic. 10. Sketch an energy diagram for a two-step exergonic reaction whose second step has a lower- energy transition state than its first step. Show on the diagram AG° for the overall reaction.
Energy 7. Consider the following energy diagram: (CH3)3C-OH (CH3)3C-ÕH₂ + HI + r a) Write the overall balanced chemical equation. Reaction coordinate (CH3)3C+ + H₂O + F b) How many steps are in the reaction mechanism? c) How many intermediates are in the reaction mechanism? d) Which step requires the most energy? (say step "X", where "X" is a number) e) CIRCLE ONE ANSWER. The overall reaction is an example of: substitution addition elimination (CH3)3C-I rearrangement
2NO2(g) + F2(g) -> NO2F(g) H°rxn = -284 kJ/molrxn NO2(g) and F2(g) can reactto produce NO2F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO2 + F2 -> NO2F + F (slow) Step 2: NO2 + F -> NO2F (fast) a.) Write a rate law for the overall reaction that is consistent with the proposed mechanism. b.) On the incomplete reaction energy diagram below, draw a curve that shows the following two details. The relative activation energies for the two elementary steps The enthalpy change of the overall reaction Can all of them be solved please, and thank you very much!
Parts 4-8
A hypothetical reaction is shown with the reaction coordinate diagram. How many steps are in the reaction mechanism? VI Reaction Progress O6
Label the energy diagram (7 bins) and indicate which reaction corresponds to the energy diagram. rate-limiting Answ transition state non-limiting transition state activation energy intermediates products starting AG° materials reaction coordinate energy 00
Use the reaction coordinate diagram to answer the below questions. Type your answers into the answer box for each question. (Watch your spelling) Energy A B C D Reaction coordinate E A) Is the reaction step going from D to F endothermic or exothermic? A F G B) Does point D represent a reactant, product, intermediate or transition state? A/ C) Which step (step 1 or step 2) is the rate determining step? A
Which species does the first transition state of the overall reaction most ressemble? What kind of transition state is this (late or early)?
A + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction. Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2 assuming c is psuedo-state-concentration overall chemical rxn is 3A+2B->2D
In comparing these two reactions, which one would occur faster via the SÃ2 mechanism and why? Reaction I CI OH- Reaction II CI 1 NH₂
Consider the following rate law: rate = k[acetone] [12]°[H*J? What effect would decreasing the concentration of acetone have on the rate of the reaction? increase decrease no effect What effect would decreasing the concentration of Ht have on the rate of the reaction? increase decrease no effect What effect would increasing the concentration of iodine have on the rate of the reaction? O increase decrease no effect

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