Iron (II) ion is oxidized by chlorine in aqueous solution, the overall reaction being:2Fe?+ (aq) + Cl2 (aq) → 2FE3+ (aq) + 2Cl- (aq)It is found experimentally that the rate of the overall reaction is decreased when either the iron (III) ion or the chloride ion concentration is increased. Is the followingmechanism consistent with the experimental observations? Explain your answer in 2-3 complete sentences. Prove by finding the rate law for the proposedmechanism.MechanismStep 1 Fe?+ (aq) + Cl2 (aq) = Fe4+ (aq) + 2Cl- (ag)(fast)Step 2 Fe+ (aq) + Fe2+ (aq) – > 2Fe3+ (ag)slow

Slow step is the rate determining step. Increase in the concentration of products decreases the rate…

Answered: Iron (II) ion is oxidized by chlorine…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 64AP

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There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?
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 plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
When enzymes are present at very low concentration, their effect on reaction rate can be described by first-order kinetics. Calculate by what factor the rate of an enzyme-catalyzed reaction changes when the enzyme concentration is changed from 1.5 107 M to 4.5 106 M.
Alcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 2530%. Women metabolize alcohol a little more slowly than men: [C2H5OH](M) 4.4102 3.3102 2.2102 Rate(moI/L/h) 2.0102 2.0102 2.0102 Determine the rate equation, the rate constant, and the overall order for this reaction.
Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecule-1s-1. Convert the following rate constants to L mol-1s-1: 3.51014 cm3 molecule-1 s-1 7.11018 cm3 molecule-1 s-1 6.11030 cm3 molecule-1s-1
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?

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