Answered: Trial 1 2 3 4 time (s) 250 135 60 120…

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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Question

how do you calculate the rate constant, k, by using the orders, a, b, and c, that you calculated above, the rate
and concentration data from Trial 1. Remember that a rate constant must have units. Write the full rate law for the reaction below including all the numbers you just calculated.

Trial
1
12
13
14
time (s)
250
135
60
120
Rate
0.00317
0.0059
0.013
0.00608
[BrO3-] (M) [H+] (M)
0.0012
0.020
0.0024
0.0012
0.0012
0.020
0.040
0.020
[1-] (M)
0.0060
0.0060
0.0060
0.012

Trail 1
=
b = 2
C = 1
b
0.00317 = K[0.0012] a [0.0201 [0.0000]°

Expert Solution

Step 1

Let the rate law :

$r = K {[B r {O_{3}}^{-}]}^{a} [H^{+}]^{b} [I^{-}] (I)$

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