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What is the half-life for a particular reaction if the rate law is rate= (1271 M*min) [A] and the initial concentration of A is 0.250 M?

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider a decomposition reaction that occurs via the following balanced chemical equation: AB2 → AB + B This reaction is first order with k = 7.7 x 10-7 s-1. What is the half-life (t1/2) of this reaction when the temperature is 1000.°C, and the initial concentration of AB2 is 0.269 M? Express your answer in units of seconds.
For the reaction 2 A + 4 B → 2 C + 4 D, what is the absolute magnitude of the rate of change for [B] when [C] is increasing at 2.0 M/s?
The first-order rate constant for the decomposition of N205, given below, at 70°C is 6.82 10-3 s. Suppose we start with 0.0200 mol of N205(g) in a volume of 5.0 L. 2 N205(g) → 4 NO2(g) + O2(g) (a) How many moles of N205 will remain after 1.5 min? mol (b) How many minutes will it take for the quantity of N205 to drop to 0.005 mol? min (c) What is the half-life of N205 at 70°C? min
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Consider this reaction: CICH, CH, CI (g) → CH,CHCI (g) +HC1 (g) At a certain temperature it obeys this rate law. rate = (0.0361 s")[CICH,CH,CI] Suppose a vessel contains CICH,CH,Cl at a concentration of 0.860M. Calculate the concentration of CICH,CH,Cl in the vessel 36.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
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