58. In some reactions there is a competition between kinetic control and thermodynamic control overproduct yields. Suppose compound A can undergo two elementary reactions to stable products:A근 Bork2A 2 Ck_2For simplicity we assume first-order kinetics for both forward and reverse reactions. We take thenumerical values k = 1 × 10° s-1, k_1 = 1 × 10? s-1, k2 = 1× 10° s-1, and k_2 = 1 × 104 s-1.(a) Calculate the equilibrium constant for the equilibriumFrom this value, give the ratio of the concentration of B to that of C at equilibrium. This is anexample of thermodynamic control.(b) In the case of kinetic control, the products are isolated (or undergo additional reaction)before the back reactions can take place. Suppose the back reactions in the preceding example(k-1 and k-2) can be ignored. Calculate the concentration ratio of B to C reached in this case.

Answered: Image /qna-images/answer/3fc66ca0-0a14-4ac1-8d4d-4a5ecaac97a8.jpg

Answered: In some reactions there is a…

In some reactions there is a competition between kinetic control and thermodynar product yields. Suppose compound A can undergo two elementary reactions to sta A근 B k-1 or A근C k_2

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...

See similar textbooks

Similar questions

Consider the following elementary reaction mechanism where both the forward and reverse reactions are important: kf1 CO+O₂ CO₂ +0 2 kr1 O+H₂O OH+OH kƒ2 kr2 kƒ3 CO+OH=CO,+H k₁.3 kf4 H+0,⇒OH+O kr 4 1. Write all chemical rate differential equations that are needed to determine the chemical evolution of the system. 2. Write all initial conditions that are needed to determine the chemical evolution of the system. 3. Is this system of rate differential equations sufficient to solve for the evolution of compositions of each chemical species? Explain, including a discussion of what else might be needed.
Derive the rate law using Steady-State Approximations N2O5 = NO2 + NO3 (K1) NO2 + NO3 = N2O5 (K-1) NO2 + NO3 = NO2 + O2 + NO (K2) NO + N2O5 = 3NO2 (K3)
The presence of a catalyst provides a reaction pathway in which the activation energy of a reaction is reduced by 70.00 kJ mol-1. . Uncatalyzed: Catalyzed: A B E₁ = 131.00 kJ - mol¹ A B E₁ = 61.00 kJ mol-¹ Determine the factor by which the catalyzed reaction is faster than the uncatalyzed reaction at 290.0 K if all other factors are equal. times faster kcat kuncat = Determine the factor by which the catalyzed reaction is faster than the uncatalyzed reaction at 338.0 K if all other factors are equal. k cat k uncat == times faster
3. What is the AH of the reaction 2KS +2K 2K,S? K+S KS AH = +32.5 kJ %3D KS+K K2S AH = +38.2 kJ %3D O +65 kJ +6 kJ +70.7 kJ +76.4 kJ
For the gas phase decomposition of 2-bromopropane,CH3CHBrCH3CH3CH=CH2 + HBrthe rate constant in s-1 has been determined at several temperatures. When ln k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.55×104 K and a y-intercept of 29.9.The value of the rate constant for the gas phase decomposition of 2-bromopropane at 675 K is _____ s-1.
The reaction of tertiary butyl bromide with hydroxide ion at 55 °C (CH3)3 CBr + OH- = (CH3)3 COH + Br- is first order in (CH3)3 CBr and first order overall. Complete the rate law for this reaction in the box below. Use the form , k ;[A]m [B]n where '1' is understood for or and concentrations taken to the zero power do not appear. Don't enter 1 for m or .n Rate =
Please answer all parts
For the gas phase decomposition of 2-bromopropane,CH3CHBrCH3CH3CH=CH2 + HBrthe rate constant in s-1 has been determined at several temperatures. When ln k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.55×104 K and a y-intercept of 29.9.The value of the rate constant for the gas phase decomposition of 2-bromopropane at 691 K is _______ s-1. (Enter your answer to one significant figure.)
Show that if A reacts to form either B or C according to elementary unimolecular reactions then Show that the half-life of A is AB or = [A]t =[A]oe-(k₁+k₂)t t1/2 or A C = In 2 k₁ + k2 Show that [B]/[C]t = k₁/k₂ for all times t. For the set of initial conditions [A]o = 1, [B]o [C]o = 0, and k₁ = 1, and k₂ = 4 plot [A], [B], and [C] as functions of time on the same graph.
Give correct handwritten answer
What is the correct mechanism number
Solve c using FOLDE (First order linear differential equation) and d