(1) L(g)=2 I(g)k-(fast, equilibrium)k2(2) I(g) +H,(g) – HI(g) + H(g)(slow)(3) H(g) + I(g)– HI(g)(fast)Which of these mechanisms are consistent with the observed rate law?O mechanism BO mechanism AO mechanism CIn 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficientto break the I–I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and thisadditional observation?O mechanism CO mechanism BO mechanism AQuestion Source: McQuarrie, Rock, And Gallogly 4e- General Chemsitry | Publisher:DIIDDF11F10F9888FBF7F5F4&56RT.YHKFM+ CO The reaction described byH, (g) + L,(g) 2 HI(g)has an experimentally determined rate law ofrate = k [H2] [I2]Some proposed mechanisms for this reaction are:Mechanism Ak1(1) H,(g) + L,(g) → 2 HI(g)(one-step reaction)Mechanism Bk1=2 I(g)k_1(1) L(g) ;(fast, equilibrium)k2(2) H, (g) + 2 I(g) 2 HI(g)(slow)Mechanism Ck1= 2 I(g)(fast, equilibrium)(1)k2(2)I(g) + H, (g) HI(g) + H(g)(slow)(3)H(g) + I(g) → HI(g)(fast)Question Sourc

The reaction described by H2 (g) + I2 (g) ---> 2HI(g)

(1) L(g)=21(g) k- (fast, equilibrium) k2 (2) I(g) +H,(g) HI(g) + H(g) (slow) k3 (3) H(g) + I(g): HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? mechanism B mechanism A mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? mechanism C mechanism B mechanism A Ouestien Sevrss: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publish

(1) L(g)=21(g) k- (fast, equilibrium) k2 (2) I(g) +H,(g) HI(g) + H(g) (slow) k3 (3) H(g) + I(g): HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? mechanism B mechanism A mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? mechanism C mechanism B mechanism A Ouestien Sevrss: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publish

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.7: Reaction Mechanisms

Problem 11.12E

See similar textbooks

Similar questions

A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
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 hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?
The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and the half-life is 30.0 s. Calculate the concentration of the reactant exactly 60 s after initiation of the reaction. How long would it take for the concentration of the reactant to drop to one-eighth its initial value? How long would it take for the concentration of the reactant to drop to 0.040 mol/L?
Gaseous azomethane, CH3N=NCH3, decomposes in a first-order reaction when heated: CH3N=NCH3(g) N2(g) + C2H6(g) The rate constant for this reaction at 600 K is 0.0216 min1. If the initial quantity of azomethane in the flask is 2.00 g, how much remains after 0.0500 hour? What mass of N2 is formed in this time?
At 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment involving this reaction: t(s) [C4H6] (mol/L) 0 0.01000 1000.. 0.00629 2000. 0.00459 3000. 0.00361 a. Determine the order of the reaction in butadiene. b. In how many seconds is the dimerization 1.0% complete? c. In how many seconds is the dimerization 10.0% complete? d. What is the half-life for the reaction if the initial concentration of butadiene is 0.0200 M? e. Use the results from this problem and Exercise 45 to calculate the activation energy for the dimerization of butadiene.