Consider the following mechanism in aqueous solutions. At 298 K the equilibrium constant for the first step is 5.75⋅10−35.75⋅10-3 k1k1 Step1: A + A −−→←−−←→ A + B k−1k-1 k2k2 Step2: B →→ P When [A] is large, the second step is slow and the first step is
Consider the following mechanism in aqueous solutions. At 298 K the equilibrium constant for the first step is 5.75⋅10−35.75⋅10-3
k1k1
Step1: A + A −−→←−−←→ A + B
k−1k-1
k2k2
Step2: B →→ P
When [A] is large, the second step is slow and the first step is fast and at equilibrium.
Under these conditions the following experimental data is gathered. The third column in the table is a check to make sure [A] is sufficiently large. The ratio should be greater than 100 when the absolute uncertainties are ±0.01±0.01 Note that as time goes on here, the assumption we are making will not work.
| Time (s) | [A] (mol L-1) | k−1[A]k2k-1[A]k2 (s) |
| 5.00 | 0.993 | 1,970 |
| 25.0 | 0.967 | 1,920 |
(a) Use the correct integrated rate law obtained by analyzing the mechanism to find a value for the rate constant k2.k2.
First calculate the effective rate constant. You need to do the proper analysis of the mechanism to find what combinations of k1k1, k−1k-1 and k2k2 give you the effective rate constant.
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