please draw the correct mechanism for this reaction Drawing the steps for an E2 or E1 mechanismAfter running various experiments, you determine that the rate law for the following reaction has a first-order dependance on theconcentration of both of the reactants.Br+XUsing this information, draw the correct mechanism in the space below.XExplanationCheckBrXXOH + BrAdd/Remove step0/5Click and drag to startdrawing a structure.2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy

Approach to solving the question: This is a simple E2 elimination reaction because the it is given…

Answered: Drawing the steps for an E2 or E1…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter13: Substitution

Section: Chapter Questions

Problem 43CTQ

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. Answer the following questions on the mechanism below. HCl + CH3CHCH2 → H+ CH;CHCICH2 fast H+ HCl → H2C1 fast H2C1 + CH3CHCICH2 → HCI+ CH3CHCICH3 slow b. Draw a reaction profile that is consistent a. What is the overall equation? What is the role of HCl in the reaction? with the mechanism. The reaction is exothermic. Reaction progress c. Determine the rate law for the mechanism. Energy
Please show your work (this is not a graded assignment)
Arrange the following compounds in order of increasing reaction rate with HNO3/H2SO4. 1. C6H5CH=O II. C6H5OCH3 III. C6H5Br IV. C6H5CH3 O I
Do you agree or disagree with this proposed mechanism? Explain.
The below reaction follows second order rate kinetics and proceeds via a bimolecular mechanism. KCNCH3B1 -» KBr + CH3CN If the concentration of potassium bromide were doubled, how many times faster would the reaction go? If the concentration of CH3Br were doubled. How much faster would the reaction go? Write the rate law for the above reaction. If [KCN] 0.5 M, [CH3Br] 0.5 M, and the relative reaction rate is 0.25 M/s, what is the rate constant? Also, what are the units of the rate constant?
Please help me to figure this out. I got 24 is that correct? Please step by step help.
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!
The 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.
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Outline a detailed mechanism for the reaction below. Identify the abbreviation for the reaction mechanism. OH H PO4
After running various experiments, you determine that the rate law for the following reaction has a first-order dependence on the concentration of the alkyl halide, and doesn't depend on the concentration of the other reactant at all. Br + H₂O + H30* + Br Using this information, draw the correct mechanism in the space below. Br Add/Remove step X G Click and drag to start drawing a structure.
2- Write step-by-step mechanism for the following reaction: Cul R1 но .*...... ....... ........

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