Consider this reaction:2N₂O5 (g) → 2N₂O4 (g) + O₂(g)At a certain temperature it obeys this rate law.= (0.291 M¹s¹) [N₂0₂]rateSuppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initialvalue. You may assume no other reaction is important.Round your answer to 2 significant digits.?SubmContinueⒸ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente80°F Partly sunny^pe here to searchBXG

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Consider this reaction: 2N₂O, (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.291 M¹.s -)[N,o, Suppose a vessel contains N₂O5 at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O5 to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. S ? X

Consider this reaction: 2N₂O, (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.291 M¹.s -)[N,o, Suppose a vessel contains N₂O5 at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O5 to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. S ? X

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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3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
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23. Consider the following reaction: 2 NO2(g) + O3(g) N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____ M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____ M/s