Consider the following mechanism for the formation of tert-butanol: (CH3) CBr(aq) (CH3), C+ (aq) (CH₂)₂C¹ (aq) + OH¯(aq) → (CH₂)¸COH(aq) 1 Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. 0 + Br (aq) yes no (1) (2) ローロ 0.0. X e

Consider the following mechanism for the formation of tert-butanol: (CH3) CBr(aq) (CH3), C+ (aq) (CH₂)₂C¹ (aq) + OH¯(aq) → (CH₂)¸COH(aq) 1 Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. 0 + Br (aq) yes no (1) (2) ローロ 0.0. X e

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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In the reaction 2 N2O5 → 4 NO2 + O2 given that the rate law is v = k[N2O5] where v is the reaction rate or reaction velocity, calculate the rate of formation of NO2 if the instantaneous rate of reaction is 1.6 x 10−6 mol L−1 s−1. Insert answers in the form x.xE±x and include units
The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
Propose a reaction pathway consisting of only a unimolecular or bimolecular steps for the 2A+B-->C+D that is consistent with the rate law rate=k(A)(B). Make sure you label which step is the rate determining step and prove that your proposed mechanism gives both the overall reaction and overall rate law. Explain the assumptions you must make in order for your mechanism to be consistent with the actual rate law.
4. The rate law for the reaction H₂ (g) + I₂ (g) → 2 HI (g) was determined to be rate = k [H₂] [1₂], which led to a simple single-step bimolecular mechanism where an H₂ molecule simply collided with an I₂ molecule. In the 1960s, though, different teams found spectroscopic evidence for this mechanism: (1) (2) (3) I₂ (g) →21 (g) H₂(g) + I (g) → H₂I (g) H₂I (g) + I (g) → 2 HI (g) (fast) (fast) (slow) Show that this mechanism is consistent with the rate law: rate = k [H₂] [1₂]. To do this, assign individual rate constants for ALL forward and reverse reactions in the mechanism (I'm guessing k₁, k-1, k2, k-2 and k3). Then show that the overall rate law from combining individual rate laws for the mechanism steps yields rate = (some combination of k's) [H₂] [1₂], and thus k= (some combination of k's). Remember that there should be no reaction intermediates in the rate law, only reactants. \
2) For each of the following reactions, list three ways in which the rate of the reaction could be increased: i) CaCO3(s) + 2HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l) ii) H₂(g) + 12(g) → 2HI(g) iii) 2H₂O₂(aq) → 2H₂O(1) + O2(g)
A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow
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Consider the following reaction: 2MnO4–(aq) + 10Br–(aq) + 16H3O+(aq) --> 2Mn2+(aq) + 5Br2(aq) + 24H2O(l) In a reaction under a certain condition, if the rate for the formation of Br2 (D[Br2]/Dt) is 1.0 x 10–5 mol ‧ L–1 ‧ s–1, what is the rate for the disappearance of 2MnO4– (-D[MnO4–]/Dt) in mol ‧ L–1 ‧ s–1 ? (A) 1.0 x 10–5 (B) 4.0 x 10–6 (C) 2.5 x 10–6 (D) 2.5 x 10–5
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
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