What is the overall reaction order of this reaction F2 + 2CIO2 → 2FCIO2? Use the given reaction rate below. EXPERIMENT [F:](M) [CIO2] (M) Rate (M/s) 1 0.10 0.010 0.0012 0.10 0.040 0.0048 3 0.20 0.010 0.0024 O a) Zero-Order Reactions O b) First-Order Reactions O c) Second-Order Reactions O d) Third-Order Reactions

What is the overall reaction order of this reaction F2 + 2CIO2 → 2FCIO2? Use the given reaction rate below. EXPERIMENT [F:](M) [CIO2] (M) Rate (M/s) 1 0.10 0.010 0.0012 0.10 0.040 0.0048 3 0.20 0.010 0.0024 O a) Zero-Order Reactions O b) First-Order Reactions O c) Second-Order Reactions O d) Third-Order Reactions

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 103QAP

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Similar questions

A certain reaction has the form aAProducts At a particular temperature, concentration versus time data were collected. A plot of 1/ [A] versus Lime (in seconds) gave a straight line with a slope of 6.90 102. What is the differential rate law for this reaction? What is the integrated rate law for this reaction? What is the value of the rate constant for this reaction? If [A]0 for this reaction is 0.100 M, what is the first half-life (in seconds)? If the original concentration (at t = 0) is 0.100 M, what is the second half-life (in seconds)?
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
a Write a rate law and an integrated rate law for a chemical reaction that follows third-order kinetics in one of the reactants. b What would you have to plot on a graph in order to get a straight line for a reaction that follows third-order kinetics?
What is the difference between average rate, initial rate, and instantaneous rate?
Derive an expression for the half-life of a a third order reaction;b a reaction whose order is =1; c a reaction whose order is 12. In these last two cases, examples are rare but known.
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
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.
Cyclobutane can decompose to form ethylene: The cyclobutane concentration can be measured as a function of time by mass spectrometry (a graph is nearby). Write an expression for the rate of reaction in terms of a changing concentration. Calculate the average rate of reaction between 10. and 30. s. Calculate the instantaneous rate of reaction after 20. s. Calculate the initial rate of reaction. Calculate the instantaneous rate of formation of ethylene 40. s after the start of the reaction.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
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.