None Choose the options below that are true. (select all that apply)Select all that apply:The rate law for a given reaction can be determined from a knowledge of the rate-determining step in thatreaction's mechanism.The rate laws of all chemical reactions can be determined directly from their net chemical equations.The rate laws of bimolecular elementary reactions are second order overall.The rate law for a given reaction can be determined from its reaction mechanism, without the accompanying ratesof each elementary step in the mechanism.

Answered: Choose the options below that are true.…

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 34QRT: When phenacyl bromide and pyridine are both dissolved in methanol, they react to form...

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Similar questions

For this reaction mechanism, write the chemical equation for the overall reaction. write the rate law for the reaction. is there a catalyst involved in this reaction? If so, what is it? identify all intermediates in the reaction. draw a reaction energy diagram for the reaction.
If you know some calculus, derive the integrated first-order rate law for the reaction by following these steps: Define the reaction rate in terms of [A]. Write the rate law in terms of [A], k, and t. Separate variables in the rate law. Integrate the rate law. Write the integrated equation in the form . Derive the half-life as was done in Section 11-3c.
. find the rate law predicted for a particular reaction mechanism.
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?
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
The type of rate law for a reaction, either the differential rate law or the integrated rate law, is usually determined by which data is easiest to collect. Explain.
Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.
When phenacyl bromide and pyridine are both dissolved in methanol, they react to form phenacylpyridinium bromide. When equal concentrations of reactants were mixed in methanol at 35 C, these data were obtained: (a) Determine the rate law for this reaction. (b) Determine the overall order of this reaction. (c) Determine the rate constant for this reaction. (d) Determine the rate constant for this reaction when the concentration of each reactant is 0.030 mol/L.
The hydrolysis of the sugar sucrose to the sugars glucose and fructose follows a first-order rate equation for the disappearance of sucrose. C12H22O11(aq)+H2O(l)C6H12O6(aq)+C6H12O6(aq) Rate =k[C12H22O11] In neutral solution, k=2.11011 at 27 C. (As indicated by the rate constant, this is a very slow reaction. In the human body, the rate of this reaction is sped up by a type of catalyst called an enzyme.) (Note: That is not a mistake in the equation—the products of the reaction, glucose and fructose, have the same molecular formulas, C6H12O6, but differ in the arrangement of the atoms in their molecules). The equilibrium constant for the reaction is 1.36105 at 27 C. What are the concentrations of glucose, fructose, and sucrose after a 0.150 M aqueous solution of sucrose has reached equilibrium? Remember that the activity of a solvent (the effective concentration) is 1.

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