The rate law for the reaction2NOB1(g)→ 2NO(g) + Br,(g)at some temperature isA[NOBI]Rate =k[NOB1]Ata. If the half-life for this reaction is 2.00 s when [NOBR].S0.900 M, calculate the value of k for this reaction.b. How much time is required for the concentration of NOBto decrease to 0.100 M?

We have given that a) t1/2 = 2 s {NOBr]0 = 0.9 M k = ? b) [NOBr]t = 0.1 M t = ?

The rate law for the reaction 2NOB1(g) 2NO(g) + Br,(g) at some temperature is A[NOBI] Rate = K[NOB1] %3D At a. If the half-life for this reaction is 2.00 s when [NOB1]o 0.900 M, calculate the value of k for this reaction. b. How much time is required for the concentration of NOBR to decrease to 0.100 M?

The rate law for the reaction 2NOB1(g) 2NO(g) + Br,(g) at some temperature is A[NOBI] Rate = K[NOB1] %3D At a. If the half-life for this reaction is 2.00 s when [NOB1]o 0.900 M, calculate the value of k for this reaction. b. How much time is required for the concentration of NOBR to decrease to 0.100 M?

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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