A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: A + B rightleftharpoons C; B + C-> D (fast) (slow) Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^ ^ 3*[D]).

A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: A + B rightleftharpoons C; B + C-> D (fast) (slow) Express your answer in terms of k and the necessary concentrations (e.g., k[A]^ ^ 3[D]).

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

Use the kinetic theory to justify the observation that the rate of a reaction in the gas phase depends on the energy of the two molecules that collide.
Explain what is meant by homogeneous and heterogeneous catalysis and give at least two examples of how industrial catalysts can be used.
Determine the rate law for the formation of oxygen predicted by this mechanism. (Assume the steady-state approximation is valid for any reaction intermediates.) k₁ CIO + CIO + M (CIO)₂ → CIOO + Cl (CIO)2 + sunlight k3 C100 + M k4 →→ Cl + O₂ 2x (C1 + 03 net: 2 033 0₂ → CIO + O₂) (this reaction occurs twice in the mechanism)
The generic reaction 2 A → products follows zero-order kinetics with a rate constant of 0.00628 M/s. What is the half-life of substance A if its original concentration is 2.23 M? Be sure to enter a unit with the answer.
Geologists can estimate the age of rocks by their uranium-238 content. The uranium is incorporated in the rock as it hardens and then decays with first-order kinetics and a half-life of 4.5 billion years. A rock is found to contain 83.0%83.0% of the amount of uranium-238 that it contained when it was formed. (The amount that the rock contained when it was formed can be deduced from the presence of the decay products of U-238U-238.) How old is the rock?
Geologists can estimate the age of rocks by their uranium-238 content. The uranium is incorporated in the rock as it hardens and then decays with first-order kinetics and a half-life of 4.5 billion years. A rock contains 83.2% of the amount of uranium- 238 that it contained when it was formed. (The amount that the rock contained when it was formed can be deduced from the presence of the decay products of U-238.) How old is the rock?
At a certain temperature the rate of this reaction is second order in ClCH2CH2Cl with a rate constant of ·0.0543M−1s−1: →ClCH2CH2Clg+CH2CHClgHClg Suppose a vessel contains ClCH2CH2Cl at a concentration of 0.710M. Calculate the concentration of ClCH2CH2Cl in the vessel 210. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M
Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO₂)² The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A B+C 2. B+D+E+C Part A What is the overall reaction? Express your answer as a chemical equation. ► View Available Hint(s) for Part A for Pardo for Part redo foPart A refor Part A keyboard shortcuts for Part A help for Part A A chemical reaction does not occur for this question. Submit Part B Which species is a reaction…
What approximation is used to determine the rate law of linear chain reactions? Justify your answer.
How might you experimentally distinguish between a first-order and second-order kinetic reaction?
The OH radical reacts with itself in a disproportionation type reaction according to the reaction: OH + OH → H2O + O This rate constant at room temperature is 2.69 x 102 M-1 s-1. If the initial concentration of OH is 2.60 x 10-5 M, what is the first half life for the reaction (in seconds)? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)
Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1