Which of the following is one of the steps in the mechanism of the reaction shown below? H+ CH3OH H20 HO. OCH3 OH CH,OH HO a) c) CH,0 OH HO. OH OCH3 H. OH CH;0 b) R R OH d) CH;OH OCH, HO, OH HOHCH3
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- For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction: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!4. Explain why the rate of formation of 1-azidopropane is different depending on which halopropane (X = F, Cl, Br, I) is used. Explain which halopropane will react fastest? ~X X = F, Cl, Br, I NaN №3 1-azidopropane
- What is an intermediate in the mechanism of the following reaction? * catalytic H,SO, но но HO HO H I-O0Determine the mechanism (SN1, SN2) of the reaction. H2O, heat -Br HO-• Br₂ Which of the following is a likely intermediate in the mechanism for the reaction given above? O O There is no intermediate, due to a concerted mechanism. Le O Br Br Bro Br Br
- The exergonic reaction below involves multiple elementary steps and one of the intermediates in the reaction is shown in square brackets. Which statement is consistent with this reaction? HCI, H2O но OH O This is a rearrangement reaction O The low energy transition state makes the reaction exergonic O The reaction has at least two transition states and the products are lower in energy than the reactants O The intermediate in the reaction must be more stable than the reactants O The reaction has one transition state, and the products are lower in energy than the reactantsWhich molecule is a reaction intermediate in the mechanism of the reaction shown below? a. OH 人士 O b. O O d. l 1. OH MgBr (2 equiv.) 2. H3O+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 a hydrocarbon solution, the gold compound (CH3)3AUPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AUPH3. The following mechanism has been proposed for the decomposition of (CH3)3AUPH3: Step 1: (CH3)3 AuPH; (CH3);Au + PH3 (fast) Step 2: (CH3)3 Au 4, C,H, + (CH;)Au (slow) Step 3: (CH3)Au + PH3 (CH3)AUPH3 (fast) (a) What is the overall reaction? (b) What are the inter- mediates in the mechanism? (c) What is the molecular- ity of each of the elementary steps? (d) What is the rate- determining step? (e) What is the rate law predicted by this mechanism? (f) What would be the effect on the reac- tion rate of adding PH3 to the solution of (CH3)3AUPH3?Outline a detailed mechanism for the reaction below. Identify the abbreviation for the reaction mechanism. OH H PO4The reaction mechanism is given below. elementary step 1 : Br2 ⇋ 2Br fast elementary step 2: H2 + Br à HBr + H slow rate determining step elementary step 3: H + Br2 à HBr + Br fast Overall reaction is H2 + Br2 à 2HBr k1 is the forward reaction rate constant of step 1, k-1 reverse reaction rate constant of step 1, k2 for reaction rate constant of step 2 and k3 for reaction rate constant of step 3. What is the molecularity of step 2? Give the chemical formula of the intermediate(s) in the reaction Deduce the rate law in terms of the reagents for the reaction using the elementary steps.