15. Use the data in the following chart to answer the questions. Initial Concentration Initial Concentration Initial Rate (mol/L-s) of A (mol/L) of B (mol/L) 0.10 0.10 1.0 × 103 0.10 0.20 2.0 x 103 0.10 0.40 4.0 x 103 0.20 0.20 1.6 x 102 0.40 0.20 1.28 x 101 a) Write the rate law equation for the reaction. b) Find the value of k. Show all work. c) What is the overall order for the reaction?

15. Use the data in the following chart to answer the questions. Initial Concentration Initial Concentration Initial Rate (mol/L-s) of A (mol/L) of B (mol/L) 0.10 0.10 1.0 × 103 0.10 0.20 2.0 x 103 0.10 0.40 4.0 x 103 0.20 0.20 1.6 x 102 0.40 0.20 1.28 x 101 a) Write the rate law equation for the reaction. b) Find the value of k. Show all work. c) What is the overall order for the reaction?

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
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. Account for the increase in reaction rate brought about by a catalyst.
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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?
Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?
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