Consider the hypothetical reaction and rate data below. Determine the form of the rate-law expression (i.e., determine the values of a and b in rate = K[A] [B] b) and also the value of the specific rate constant, k. Which of the answers below would be the initial rate of reaction for [A] initial = 0.40 M and [B] initial = 0.10 M? 3A + 2B →→→ Products Run 1 2 3 O a.4.8x 10-4 Mes 1. O b.1.2x 10-3 Mes-1 Oc3.4 x 10-3 Mos-1 Od-6.4×10-3 MS-1 O e 1.6x 10-4 Mos-1 [A] initial 0.10 M 0.20 M 0.30 M [B] initial 0.10 M 0.30 M 0.10 M Initial Rate of Reaction (moles per liter per second) 4.0x 10-4 4.8 x 10-3 3.6× 10-3

Consider the hypothetical reaction and rate data below. Determine the form of the rate-law expression (i.e., determine the values of a and b in rate = K[A] [B] b) and also the value of the specific rate constant, k. Which of the answers below would be the initial rate of reaction for [A] initial = 0.40 M and [B] initial = 0.10 M? 3A + 2B →→→ Products Run 1 2 3 O a.4.8x 10-4 Mes 1. O b.1.2x 10-3 Mes-1 Oc3.4 x 10-3 Mos-1 Od-6.4×10-3 MS-1 O e 1.6x 10-4 Mos-1 [A] initial 0.10 M 0.20 M 0.30 M [B] initial 0.10 M 0.30 M 0.10 M Initial Rate of Reaction (moles per liter per second) 4.0x 10-4 4.8 x 10-3 3.6× 10-3

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

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