6.) The rate law for the reaction below is found experimentally to be Rate = k[N2O5] and the rate constant, k = 6.20 × 10s-. SHOW ALL WORK! %3D 2 N2O5 (g) → 4 NO2 (g) + O2 (g) a. Determine the time for the concentration of N2O5 to go from 0.400 M to 0.200 M. b. if [N2O5]o = 0.400 M, calculate [N2O5] at t = 60.0 min.

6.) The rate law for the reaction below is found experimentally to be Rate = k[N2O5] and the rate constant, k = 6.20 × 10s-. SHOW ALL WORK! %3D 2 N2O5 (g) → 4 NO2 (g) + O2 (g) a. Determine the time for the concentration of N2O5 to go from 0.400 M to 0.200 M. b. if [N2O5]o = 0.400 M, calculate [N2O5] at t = 60.0 min.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.18P

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Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
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One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
For the reaction 5Br(aq)+BrO3(aq)+6 H+(aq)3Br2(aq)+3H2O It was found that at a particular instant, bromine was being formed at the rate of 0.029 mol/L s. At that instant, at what rate (a) are the hydrogen ions being consumed? (b) is water being formed? (c) are the bromide ions being consumed?
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For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
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