Multiple Choice
What is the overall reaction order for the following rate law: Rate = k[A][B][C]?
15. Chemical Kinetics
Rate Law
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What is the rate law for the reaction A → B if the rate constant, k, is 0.25 M⁻¹ s⁻¹ at 75 °C?
A
Rate = k[B]²
B
Rate = k[B]
C
Rate = k[A]
D
Rate = k[A]²
Verified step by step guidance1
Identify the general form of the rate law for a reaction: Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B, respectively.
Since the reaction is A → B, the rate law will only involve the concentration of A, as B is a product and does not appear in the rate law.
Examine the given rate constant units, M⁻¹ s⁻¹. These units suggest a second-order reaction overall, as the units of k for a second-order reaction are typically M⁻¹ s⁻¹.
Since the reaction involves only one reactant, A, and the overall order is second, the rate law must be Rate = k[A]².
Conclude that the correct rate law for the reaction A → B is Rate = k[A]², as it matches the order suggested by the units of the rate constant.
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