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Date: 23-9-2018
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Date: 19-12-2020
639
Date: 23-9-2018
80
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We have just seen that first-, second-, and zero-order reactions all have unique, integrated rate-law equations that allow us to plot them as a straight line (y = mx + b) (Table 1.1 “Integrated Rate Law Summary”). When presented with experimental concentration–time data, we can determine the order by simply plotting the data in different ways to obtain a straight line.
Table 1.1 Integrated Rate Law Summary
Example 1
The following data were obtained for the reaction 3 A → 2 B:
Time, s |
0 |
1 |
10 |
11 |
20 |
[A], M |
0.200 |
0.0282 |
0.0116 |
0.0106 |
0.008 |
Determine the order of the reaction.
Solution
We can plot the characteristic kinetic plots of zero-, first-, and second-order reactions to determine which will give a straight line.
Time, s |
[A], mol L-1 |
ln [A] |
1/[A], L mol-1 |
0 |
0.200 |
-1.61 |
1.00 |
1 |
0.0282 |
-3.17 |
31.1 |
10 |
0.0116 |
-4.16 |
64.1 |
11 |
0.0106 |
-4.11 |
94.3 |
20 |
0.008 |
-4.83 |
121 |
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