Question 16 Consider the following reaction and its corresponding rate law to answer the question. 2 NO (g) + O2 (g) 2 NO2 (9) rate = 1.15x103 M2s-1 [NO]?1O2] What is the initial rate of the reaction when the concentration of NO = 0.15 M and the concentration of O2 = 0.35 M? O 8.1x102 M/s O 5.4x10-4 M/s O 5.6x10-3 M/s O 9.1 M/s O 18 M/s

Question 16 Consider the following reaction and its corresponding rate law to answer the question. 2 NO (g) + O2 (g) 2 NO2 (9) rate = 1.15x103 M2s-1 [NO]?1O2] What is the initial rate of the reaction when the concentration of NO = 0.15 M and the concentration of O2 = 0.35 M? O 8.1x102 M/s O 5.4x10-4 M/s O 5.6x10-3 M/s O 9.1 M/s O 18 M/s

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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The reaction: 2 N2O5(g) 4 NO2(g) + O2(g) rate = K [N205]? %3D If the half-life for this reaction is 43.9 minutes, and the original concentration is 0.35 M what is the rate constant, (k)? O 2.32 x 10-3 M.s O 1.32x 10-3 M.s O 1.085 x 10-3M's1 O 1.085 x 10-3 M.s
1c
How will each of the following affect the rate of the reaction, CO(g) + NO2(g) → CO2(g) + NO(g), if the rate law for the reaction is rate = k [NO2] [CO]? (a) increasing the pressure of NO2 from 0.4 atm to 0.8 atm (increases or decreases) The rate ___?^___ by a factor of ___?___. (b) increasing the concentration of CO from 0.04 M to 0.08 M (increases or decreases) The rate ___?^___ by a factor of ___?___.
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Consider the balanced reaction below. 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g) a) Write the relative rate expression for the reaction (including each of the reactants and products). b) If the rate of N2H4 consumption is 0.50 M/s, what is the rate of N2 production? Show your work or explain your reasoning.
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Question 13 of 32 Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is Rate [A], (M) [B], (M) (M/s) A) Rate = k[A][B] 0.100 2.50 0.460 B) Rate = k[B] C) Rate = k[A]°[B] 0.200 2.50 0.920 D) Rate = k[A] 0.300 1.25 1.38 "pe here to search