The reactionH3C-1 OHH3C-OH+rmay go by either of the following mechanisms:I)H3C-1H3C++r(slow)H3C++ OH ® H3C-OH(fast)orII)H3C-1+ OHH3C-OH+I*If the first mechanism were correct, what would be the rate law?Rate = K[H3C-1]Rate =K[H3C-1][OH]Rate = k[H3C-1][OH-]2Rate =K[H3C][OH]Rate = K[H3C+]

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Answered: The reaction H3C-1 OHH3C-OH+r may go by…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine the rate law
A: Consider the following reaction: N2H5+ + 4 Fe(CN)63- --> N2(g) + 5 H+ + 4 Fe(CN)64- Based on just this information, which species concentration(s) could most likely be in the rate law? (Check ALL correct answers.) Group of answer choices Fe(CN)64- Fe(CN)63- N2H5+ N2(g) H+ B: Consider the following reaction: 2 C19H16O --> C38H32O2, also written as: 2 Monomer --> Dimer Given the following kinetics plot, what is the rate order with respect to Monomer disappearance? Group of answer choices 2nd 3rd Zero 1st
Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.
The reaction, NO₂Cl(g) + CI(g) -> NO2(g) + Cl₂(g), was found to be first order in each of the two reactants and second order overall. The rate law is therefore rate = k[NO₂]² rate = k[NO₂][ Cl₂] rate = k[CI] rate = K[NO₂CI][CI][NO₂][C1₂] rate = K[NO₂CI][CI]
Determine the rate law for the reaction, 2IC1 + H2 = I, + 2HCi, from the following initial rate data: Initial Rate(Ms') 2.04x102 4.08x102 2.55x103 5.09x103 [H,], [ICI], 0.250 0.500 0.500 0.500 0.125 0.125 0.125 0.250 A) R = k[IC1]? В) R = k[H2]? C) R = k[ICI][H_]? D) R = k[ICl][H,] E) R = k[ICI]°[H¿] 000
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Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO₂)² The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A B+C 2. B+D+E+C Part A What is the overall reaction? Express your answer as a chemical equation. ► View Available Hint(s) for Part A for Pardo for Part redo foPart A refor Part A keyboard shortcuts for Part A help for Part A A chemical reaction does not occur for this question. Submit Part B Which species is a reaction…
For the reaction H2(g) + C2H4(g) ⟶⟶C2H6(g) A series of experiments were conducted as sown in the Table. If the rate law were found to be : rate = k[H2][C2H4] what is the missing initial rate (marked with a "?" in the Table)?
2 NO (g) + O₂ (g) --> 2 NO2 (g) The proposed mechanism for the reaction above is 1) NO (g) + NO (g) --> N₂O2(g) 2) N₂O2 (g) + O2 (g) --> 2 NO2 (g) Write the rate law for the mechanism if the first step is fast and the second step is slow.
We have the following elementary reactions: A → M + C with the rate constant k1 M + C → A with the rate constant k-1 M + B → P with the rate constant k2 Answer the following questions: 1)Y ou must write down the time derivatives of the concentrations for A, C, M, B and P. This means that you must determine d[X]/dt for all five compounds, where X is one of the compounds A, C, M, B and P. 2) You must show that the reaction rate can be rewritten d [P]/dt = (k1k2)/(k-1[C]+k2[B]) You must assume that you can use the steady state approximation for the concentration of M. 3) You need to examine the expression for the reaction rate: d [P]/dt = (k1k2)/(k-1[C]+k2[B]) for two situations: i) k-1[C]>> k2 [B] ii)k-1 [C]<< k2 [B] and state which elementary reactions are rate-determining in the two situations.
1

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