Use the following data set for questions 3 and 4:A(aq) + B(aq) → ProductsRxn #[A][B]Rate of Loss of A10.120.108.4 x 10-60.120.201.7 x 10-50.240.103.4 x 10-53. Determine the orders of reaction (m and n) for reactants A and B. Explain how you came to thisconclusion or show your work.4.Determine the rate constant (k) for the reaction above.

(3) Rate law of the reaction is,

Answered: Use the following data set for…

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

Section: Chapter Questions

Problem 60QRT

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Why awe elementary reactions involving three or more reactants very uncommon?
Which one of these reactions would be best classified as irreversible? a) FeCO3(s) ⇌ Fe2+(aq) + CO32-(aq) K = 2.1 × 10-11 b) HC2H3O2(aq) + OH-(aq) ⇌ C2H3O2-(aq) + H2O(l) K = 1.8 × 10^9 c) Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) K = 215 d) 2SO2(g) + O2(g) ⇌ 2SO3(g) K = 4.32
Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.
how reaction rate increases in pressure cooking because of collision theory and energy potential diagrams : how the rate of reaction is affected by temperature, surface area, nature of reactants, concentration, etc. by using collision theory? (use Hess’s Law, Le Châtelier’s Principle, or Kinetic Molecular Theory to explain in increasing rate of reaction and relevance by including all 4 required subtopics )
What reaction is SeCI6 + O2 > SeO2 + 3CI2
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Ozone can oxidize HSO3^1-(aq) as represented below: HSO3^-(aq)+03(aq)---> HSO4^-(aq) +02(g) A solution is prepared in which the initial concentration of HSO3^1- (aq)(6.4x10^-4M) is much larger than that of O3(aq)(1.0x10^-5M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below: (see attached image) iii)Considering the relative concentration of the reactants, briefly explain why the data in the graph are also consistent with the following rate law: Rate=k1[O3][HSO3^1-] iv)Briefly describe an experiment that could provide evidence to support the rate law given in part (diii)
Ozone can oxidize HSO3^1-(aq) as represented below: HS03^-1(aq)+03(aq)-->HS04^-(aq)+02(g) A solution is prepared in which the initial concentration of HSO3^1-(aq)(6.4x10^-4 M) is much larger than that of O3(aq)(1.0x10^-5 M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below: (see attached image) The data are consistent with the following rate law: Rate = k1[O3] i) Based on the graph, determine the half-life of the reaction ii) Determine the value of the rate constant k1 for the rate law. Include units
Use the following reaction and information to answer a and b. 2ClO2(aq)+2OH-(aq)-->ClO-(aq)+Cl2-(aq)+H2O(l) [ClO2](M) [OH-](M) Initial rate (M/s) 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 a. What is the order of this reaction in respect to ClO2, with respect to OH-, and the overall order? Assume the rate law has the form rate=k[ClO2]a[OH-]b b. What is the value of the rate constant? Include the units and why the unit make sense.
For the reversible, one-step reaction A + A * k_{1}/k_{-1} * B + C the rate constant for the forward reaction, k_{1} , is 279 L* mol^ -1 * min^ -1 and the rate constant for the reverse reaction, k_{1} is 355Lmo * l ^ - 1 * mi * n ^ - 1 at a given temperature . The activation energy for the forward reaction is 43.3kJmo * l ^ - 1 whereas the activation energy for the reverse reaction is 22.8kJmo * l ^ - 1Determine the equilibrium constant, K, of this reaction.
For the reversible, one-step reaction A + A * k_{1}/k_{-1} * B + C the rate constant for the forward reaction, k_{1} , is 279 L* mol^ -1 * min^ -1 and the rate constant for the reverse reaction, k_{1} is 355Lmo * l ^ - 1 * mi * n ^ - 1 at a given temperature . The activation energy for the forward reaction is 43.3kJmo * l ^ - 1 whereas the activation energy for the reverse reaction is 22.8kJmo * l ^ - 1

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