Write the rate law for the following reaction given that the order of A = 2, B = 1, and C = 0. A + B + C ———> D + E If the concentration of C is doubled, what will happen to the rate of the reaction?

The rate law is:

Doubling the concentration of C will have no effect on the rate of the reaction.

Explanation:

We want to write the rate law for the reaction:

Where the order of A, B, and C are 2, 1, and 0, respectively.

The rate law will have the form:

Where m, n, and p are their respective order of reactions.

Hence, the rate law is:

Because the order of reaction to C is 0, changing its concentration will have no effect on the rate law.

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