Consider this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) - At a certain temperature it obeys this rate law. rate = (0.00246 s−¹)[C1₂05] S Suppose a vessel contains Cl₂O5 at a concentration of 0.500M. Calculate the concentration of Cl₂O5 in the vessel 360. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. | |м

Consider this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) - At a certain temperature it obeys this rate law. rate = (0.00246 s−¹)[C1₂05] S Suppose a vessel contains Cl₂O5 at a concentration of 0.500M. Calculate the concentration of Cl₂O5 in the vessel 360. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. | |м

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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59.)
TIA
Consider the reaction for the formation of ammonia, NH3: N2(g) + 3 H2(g) --> 2 NH3(g) Which is the correct rate expression for this reaction?
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
The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results: Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s) 1 0.00532 0.00532 0.230 2 0.00532 0.0106 0.458 3 0.0106 0.00532 0.458 4 0.0106 0.0106 0.912 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)]Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2Rate = k [HBr(g)] [O2(g)]3Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of HBr(g) is 0.00533 M and that of O2(g) is 0.0145 M if the temperature is the same as that used to obtain the data shown above? M/s