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The rate law for a reaction is expressed as k multiplied by the concentration of A raised to the power of 1 and the concentration of B raised to the power of 2. Which of the following correctly represents this rate law?

1. The rate is given by k times [A] raised to the power of 1 and [B] raised to the power of 2.
2. For a reaction of first order, the half-life is calculated as 0.693 divided by k, which equals 0.693 × 10^−3 s^−1 = 1386.
3. Doubling the concentration of A causes the rate to double, indicating the reaction is first order with respect to A.
4. Doubling the concentrations of both A and B results in an 8-fold increase in the rate, showing the reaction is second order with respect to B.

Correct answer: The rate is given by k times [A] raised to the power of 1 and [B] raised to the power of 2.

Solution

The given rate law matches the description in option A, which directly states the rate equation as Rate = k[A]^1[B]^2. This is consistent with the provided reaction order details.

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