**Question**: The following chemical transformations involve multistep mechanisms. Please write a reasonable mechanism for each transformation and label each elementary step. **Transcription of Reaction Mechanism** **Chemical Reaction:** Starting Material: - 2-butanone (C4H8O) Reagents: - 1. Strong base "B" - 2. Bromoethane (C2H5Br) Product: - 4-heptanone (C7H14O) Byproducts: - HB - Br- **Mechanism Explanation:** 1. **Deprotonation Step:** - The strong base "B" abstracts a hydrogen ion from the methyl group at position 2 of butanone, generating an enolate ion. 2. **Alkylation Step:** - The enolate ion acts as a nucleophile and attacks the electrophilic carbon in bromoethane, leading to the substitution and formation of a new C-C bond. This produces 4-heptanone as the main product while generating hydrogen bromide (HB) and bromide ion (Br-) as byproducts. This reaction illustrates a typical alkylation of enolates using a strong base to form ketones from smaller ketones and alkyl halides.

Parts A - D.

Consider the following reaction. From the given choices of intermediates, choose the 5 related to this reaction and put them in order to describe the complete mechanism (all the steps involved) for this reaction.

WS-2.10: Draw the mechanism and list the elementary steps for reaction. H₂O TfOH U

for the reaction 2Fe2 + + H2O2 = 2Fe3 + + 2OH- the rate of formation of Fe3 + ions is given by the kinetic equation V = k [Fe2 +] [H2O2] .Propose a mechanism for the reaction and show the order for each elementary reaction.

The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH → (CH3)3COH + Br Experiment [(CH3)3CB1],, M [OH], M Initial Rate, Ms-1 1 0.890 1.50x10-3 1.50x10-3 3.01x10-3 3.01x10-3 0.118 0.118 2 1.78 0.890 1.78 3 0.237 4 0.237 Complete the rate law for this reaction in the box below. Use the form k[A]j™[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI

The activation energy for the gas phase decomposition of cyclobutane is 262 kJ. (CH₂) 4- →2 C₂H4 The rate constant at 721 K is 0.000401 /s. The rate constant will be 0.00338/s at K.