In order to find the rate constant k, we need to set up the rate law first. The problem here is that we don't know the reaction order of each reactant. Remember that the rate law only cares about the reactant and not the products. So what we have to do is to set up the rate law as shown below where x would be the order of A and y the order of B. We can then just solve for x and y later using the data given.
Using the given data, determine the rate constant of this reaction.
A + 2B → C + D
Trial [A](M) [B](M) RATE (M/s)
1 .330 .280 0.0236
2 .30 .560 0.0236
3 .660 .280 0.0944
k=? the units are M-1 s-1
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