29-24. A proposed mechanism for the thermal decomposition of acetaldehydeCH,CHO(g)CH₁(g) + CO(g)CH,CHO(g)TyCH3(g) + CH3CHO(g)CH,CO(g)CH3(g) + CHO(g)(1)CH2(g) +CH,CO(g)(2)CH3(g) + CO(g)(3)2 CH₁(g)C₂H6(4)Is this reaction a chain reaction? If so, identify the initiation, propagation, inhibition, andtermination step(s). Determine the rate laws for CH₁(g), CH3(g), and CH3CO(g). Showthat if you assume the steady-state approximation for the intermediate species, CH3(g) andCH3CO(g), the rate law for methane formation is given byd[CH]dt1/2(1) K, CH, CHOP/22k,

The proposed mechanism for the thermal decomposition of acetaldehyde involves several steps and…

Answered: 29-24. A proposed mechanism for the…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section14.7: Reaction Mechanisms

Problem 1.2ACP

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a plausible mechanism (i) MeCCLi (ii) BRCH 2COME (ii) CH 3CO2H
Carbonic Anhydrase or carbonic dehydratase is a family of metalloenzymes containingzinc (Zn2+) ion in its active site. Carbonic anhydrase can greatly increase the rate of thisreaction, reaching a reaction rate of 104 - 106 per second. It is defined as the enzyme found inred blood cells, other parts of animals and plants, that breaks down carbonic acid with carbondioxide and water.CO2(g) + H2O(l) → H2CO3(aq)For the carbonic anhydrase activity specified by the equation above, evaluate the standardreaction Gibbs energy at 25 °C?
The mechanism for the reaction described by nust. A common d(a stronger whch ont of ice prhct NO,(g) + CO(g) → CO,(g) + NO(g) coor on be c is suggested to be (1) 2NO,(g) –→ NO,(g) + NO(g) k1 -> k2 (2) NO,(g) + CO(g) → NO,(g) + CO,(g) d[CO2] k[NO2]? %3D The experimental rate law for the production of [CO2] = k1 [NO2J² or dt d[NO3] 0 ), is this a valid mechanism? i.e show Assuming that [NO3] is governed by a steady state ( dt that using elementary reactions 1 and 2, the experimental rate law can found. (Hint write out all the ways d[NO3] = ? d[C02] = ? ) %3| and %3D dt that [NO3] and [CO2] are created and destroyed, dt owing clecre cel at 25 C NiC C)Cu a062 0.62 V 0.00 V 4. 460 V
Although CH4 reacts with Cl2 to form CH3Cl and HCl, the corresponding reaction of CH4 with I2 does not occur at an appreciable rate, even though the I–I bond is much weaker than the Cl–Cl bond. Explain why this is so.
1-Bromobutane reacts with water to form 1-butanol according to the following equation. C4H,Br(aq) + 2 H20(1) → C¿H,OH(aq) + H30*(aq) + Br¯(aq) The following is a proposed mechanism for the reaction. C4H9B1(aq) → C4H,*(aq) + Br¯(aq) C4H,*(aq) + H,0(1) → C4H3OH,*(aq) C,H,OH,*(aq) + H,0() – CH,OH(aq) + H30*(aq) slow fast fast Determine the overall rate law for this proposed mechanism. (Rate expressions take the general form: rate = k. [A]ª . [B]°.) chemPad Help Greek - Rate=k[C4H9B1][H2o²] Rate=k[C_4H_9Br][H_2O^2] Remember that answers are case-sensitive. Your answer contains an incorrect or incomplete chemical formula.
According to the mechanism given in the degradation of 12- catalyzed acetaldehyde, subtract the rate expression based only on the rate constants and 12 and acetaldehyde concentration. Note: Apply the steady-state hypothesis for I, СНЗСО and CНЗ. k 21 2 k1 k2 I+CH,CHO->HI+CH,CO k3 CH,СО СH, + CO →CH, +CO CH, + HI — kyСH, +I →CH4
6. Consider the decomposition of perbenzoic acid in water: 2 C6H5CO3(aq) → 2 C₂H5COOH(aq) + O₂(g). The reaction may proceed according to the following mechanism: C6H5CO3H k₁ k₁ C6H5CO3 + H* k₂ C6H5CO3H + C6H5CO3 → O₂ + С6H5CO₂ + C₂H5COOH Assuming that the second step is rate-limiting, and the first step in the reaction satisfies the pre-equilibrium condition, determine the rate of formation of O₂. Assume the pH remains constant throughout the reaction. Would the rate of reaction increase or decrease with a more acidic pH?
The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.
Temperature effect on the degradation of a multisulfa preparation was evaluated at 60 and 70°C. If the first-order reaction rate constants responsible for the degradation at these two temperatures were 8.2 x 10-4 and 1.96 x 10-3 hr-1, Calculate the activation energy, Ea, for this drug in this temperature range (in kcal/mole). (The gas constant; R = 1.987 cal/deg mole):
The acid-catalysed conversion of γ-hydroxybutyric acid (GHBA) into its lactone, γ-butyrolactone (GBL) is a reversible reaction. The GHBA to GBL forward reaction is first-order with respect to the GHBA concentration; the GBL to GHBA reverse reaction is first-order with respect to the GBL concentration. An experimental study of the kinetics of this reaction was undertaken in 0.2 mol L-1hydrochloric acid (HCl) at 298 K. The initial concentration of GHBA was 18.23 × 10-3mol L-1 . The concentration of GBL in solution was followed as a function of time (t), as indicated in Table B.3: Time/min 0 21 36 50 65 80 100 ∞ GBL Concentration / 10-3 L-1 0 2.41 3.73 4.96 6.10 7.08 8.11 13.28 Use the data in Table B.3 to determine the equilibrium constant and the first-order rate constants for both forward and reverse reactions.
What Is the Chemical Equation for this mechanism?
Our body obtains energy from the combustion of glucose. During this process, glycerate is transformed first into pyruvate. This reaction has an activation energy close to 44 kJ. Estimate how many times faster this reaction is when someone has a high fever close to 106 F (41 oC) compared to its rate at normal body temperature (98.6 F; 37 oC). Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b с d 31% faster 11% faster 24% faster 259% faster Your answer

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