Answered: An experiment followed the…

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

An experiment followed the decomposition of nitrogen dioxide to nitrogen monoxide and oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Calculate rate constant value.

Time(sec)	[NO₂](M)
0.0	0.01000
50.0	0.00787
100.0	0.00649
200.0	0.00481
300.0	0.00380

Expert Solution

Step 1

To check the order of the reaction, let's assume the reaction is 1st order.

The rate equation for 1st order reaction is,

$kt = \ln \frac{A_{0}}{A_{t}} k = rate constant . A_{0} = initial concentration A_{t} = final concentration t = time .$

For time = 100s, the rate constant, For time =200s, the rate constant,

$k \times 100 = \ln \frac{0.01}{0.00649} k = rate constant . A_{0} = 0.01 A_{t} = 0.00649 t = 100 s$ $k \times 200 = \ln \frac{0.01}{0.00481} k = rate constant . A_{0} = 0.01 A_{t} = 0.00481 t = 200 s . S o, k = \frac{2.07900}{200} = 0.0104$

So, $k = \frac{0.432}{100} = 0.00432$

we can see they both can't generate the same rate constant value. it is not a 1st order reaction.

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