2. Calculate the branching ratio of the reaction of the methyl peroxy radical with either HO, NO298K) (note: rate constant can be found in the tropospheric chemistry pptCH,O,+NO-HCHO+HO, + NO,CH₂O+HO, CH₂00H +0₂when the concentration of hydroperoxyl radical is DH01-1.5 x 10 molecules and thenitrogen oxide maxing ratio of 10 ppbwhen the concentration of hydroperoxyl radicalis [H0] +1.5x10 molecules cm" and thenitrogen oxide mixing ratio of 30 pUnder which condition do you expect more formaldehyde to be produced and why

Here's the breakdown of how to solve this problem, along with the answers:Understanding the…

Answered: 2. Calculate the branching ratio of the…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.49PAE: The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by...

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The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
1. Discuss the conditions under which the expression dIP kakpla]? kp+ka[A] for the effective rate dt constant of a unimolecular reaction according to the L-H mechanism results in a (a) first- order, or (b) second-order rate law.
What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1:. A+B Step 2: B+C → D (slow) C (fast) Express your answer in terms of k and the necessary concentrations (e.g., k* [A] ^3*[D]). > View Available Hint(s) nV ΑΣφ 5E.. rate =
In a temperature-jump experiment to investigate the kinetics of an isomerization reaction that is first-order in both directions, the relaxation t ime was measured as 27.6 μS. The rate constant for the forward reaction is known to be 12.4 ms-1. Ca lcu late the rate constant for the reverse reaction.
The rate law v=(kr1[A][B])/(kr2 + kr3[B]1/2) was established in a series of experiments. Identify the conditions under which (i) an order with respect to A, (ii) an order with respect to B, and (iii) an overall order, can be assigned.
5. What is the value for the rate constant, k? k = k'/1* = k = k"/0.5* = kavg r = k[OH°]*[ C25H3„N,'J" [OH] C2H,„N;'] r = 303
Which of the following rate law expressions is most likely to have the units of rate constant equal to M-3 sec1. a. Rate = k (A] [B2 b. Rate = k (A)2 [B}2 (c)? OC. Rate = k (A) [B]² (C] d. Rate = k (A] [B) e. Rate = k (A] [B)2 (c?
2. Czarnowski and H.J. Schuhmacher (Chem. Phys. Lett. 17, 235 (1972)) suggested the following mechanism for the thermal decomposition of F2O in the reaction 2 F20(g) → 2 F2(g) + O2(g): 1) F2O+ F2O →F+OF + F2O : ka ko ke kd 2) F+F20 → F2 + OF: 3) OF + OF → 02 + F + F : 4) F+F+ F2O→ F2 + F2O: Use the steady-state approximation to find the rate law of this reaction.
Give the equation for quantum yield j. rate of formation of the singlet state rate of ith decay mechanism rate of ith decay mechanism rate of removal of the singlet state rate of ith decay mechanism rate of formation of the singlet state rate of removal of the singlet state rate of ith decay mechanism Step 4 of 6 Give the quantum yield ;. (Use the following as necessary: kj, k1, k2, k3, and t.) k1 + k, + k = ki 3 k1 + k2 + k3 Recalling the relationship between the overall rate constant, k, and the mean lifetime, T, give the quantum yield D; in terms of T and Tj. (Use the following as necessary: T and T;) i Step 5 of 6 (c) If T1 = 1×10-7 s, T2 = 4x10-8 s, and T3 = 1x10-8 s, calculate the lifetime of the singlet state and the quantum yield for the path that has T2. (Enter an unrounded value with at least 3 digits.) 1 using the equation given in (b). Calculate = 7.407e-9 s-1 Solve for T, the lifetime of the singlet state. T = .185175 X S Submit
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

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