![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_largeCoverImage.gif)
Consider the zero-, first-, and second-order integrated rate laws. If you have concentration versus time data for some species in a reaction, what plots would you make to “prove” a reaction is either zero, first, or second order? How would the rate constant, k, be determined from such a plot? What does the y-intercept equal in each plot? When a rate law contains the concentration of two or more species, how can plots be used to determine k and the orders of the species in the rate law?
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 12 Solutions
Chemistry
Additional Science Textbook Solutions
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Chemistry & Chemical Reactivity
Basic Chemistry (5th Edition)
Chemistry by OpenStax (2015-05-04)
Essential Organic Chemistry (3rd Edition)
General Chemistry: Principles and Modern Applications (11th Edition)
- 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?arrow_forwardIsomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?arrow_forwardBased on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?arrow_forward
- 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.arrow_forwardThe Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardThe decomposition of many substances on the surface of a heterogeneous catalyst shows the following behavior: How do you account for the rate law changing from first order to zero order in the concentration of reactant?arrow_forward
- Kinetics II You and a friend are working together in order to obtain as much kinetic information as possible about the reaction A(g)B(g)+C(g). One thing you know before performing the experiments is that the reaction is zero order, first order, or second order with respect to A. Your friend goes off, runs the experiment, and brings back the following graph. a After studying the curve of the graph, she declares that the reaction is second order, with a corresponding rate law of Rate = k[A]2. Judging solely on the basis of the information presented in this plot, is she correct in her statement that the reaction must be second order? Here are some data collected from her experiment: Time (s) [A] 0.0 1.0 1.0 0.14 3.0 2.5 103 5.0 4.5 105 7.0 8.3 107 b The half-life of the reaction is 0.35 s. Do these data support the reaction being second order, or is it something else? Try to reach a conclusive answer without graphing the data. c What is the rate constant for the reaction? d The mechanism for this reaction is found to be a two-step process, with intermediates X and Y. The first step of the reaction is the rate-determining step. Write a possible mechanism for the reaction. e You perform additional experiments and find that the rate constant doubles in value when you increase the temperature by 10oC. Your lab partner doesnt understand why the rate constant changes in this manner. What could you say to your partner to help her understand? Feel free to use figures and pictures as part of your explanation.arrow_forwardChlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3 and ClO2 ions. 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the rate constant.arrow_forwardMany 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.arrow_forward
- (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?arrow_forwardAt 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardFor the reaction A+BC, explain at least two ways in which the rate law could be zero order in chemical A.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199023/9781285199023_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)