The data below show the concentration of ABversus time for the
following reaction:
AB(g)→A(g)+B(g)
Time (s) | [AB] (M) |
0 | 0.950 |
50 | 0.459 |
100 | 0.302 |
150 | 0.225 |
200 | 0.180 |
250 | 0.149 |
300 | 0.128 |
350 | 0.112 |
400 | 0.0994 |
450 | 0.0894 |
500 | 0.0812 |
Determine the order of the reaction.
Solution
Easiest way to determine the order of the reaction in this case is to plot the graph concentration of [AB] to the time in seconds.
Refer attached excel file.
Conclusion:
We don’t have any data about the rate of reaction. So, we can only assume about the order of the reaction.
As shown in both graphs, we can say that it is second order reaction as log[AB] vs Time did not produce a straight line. It also means that there are some factors such as concentration of product which are affecting the rate of reaction. Underlining the fact that it is Second order reaction.
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