The following reaction is second-order in A and first-order in B: 2 A+B → A₂B What is the reaction rate if k = 2.55 M-²s¹ and [A] = 1.60 M [B] = 0.70 M? Hint: Write down the correct differential rate law based on the order with respect to A and B, then plug in the concentrations and k to calculate rate (R). Your Answer: Answer units

The following reaction is second-order in A and first-order in B: 2 A+B → A₂B What is the reaction rate if k = 2.55 M-²s¹ and [A] = 1.60 M [B] = 0.70 M? Hint: Write down the correct differential rate law based on the order with respect to A and B, then plug in the concentrations and k to calculate rate (R). Your Answer: Answer units

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.27E: Derive an expression for the half-life of a a third order reaction;b a reaction whose order is =1; c...

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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?
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Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
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