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When you find the ratio between Rate 1 and Rate 4, you will see that [C] will be in zeroth order. That means that now the differential rate law is k[A][B]. Now, when finding the orders of A and B, you don't need to take into account [C] because the reaction does not depend on the concentration of [C].
In figuring out the answer, you would see that the concentration of C would be changing, but you do not take it into account since it is a zero order. The differential rate law would instead be rate = k[A][B] instead, so this way, you are able to focus on the differences between each experiment from concentrations of A and B. This would make analysis much more straightforward in comparison so you're able to determine the orders for each.
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