A reaction that involves reactants A and B is found to occur in the one-step mechanism: 2 A+B ⟶A

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A reaction that involves reactants A and B is found to occur...

A reaction that involves reactants $\mathrm{A}$ and $\mathrm{B}$ is found to occur in the one-step mechanism: $2 \mathrm{A}+\mathrm{B} \longrightarrow \mathrm{A}_{2} \mathrm{B}$ Write the rate law for this reaction, and predict the effect of doubling the concentration of either reactant on the overall reaction rate. (Hint: See Sample Problem C.)

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Key Concepts

Elementary Reaction

An elementary reaction is a single-step process where the reactants convert to products in one collision event without any intermediate steps. Because it occurs in one step, the rate law can be directly deduced from the stoichiometry of the reaction.

Rate Law

The rate law is an expression that relates the rate of a chemical reaction to the concentrations of its reactants. In an elementary reaction, the exponents of the reactant concentrations in the rate law correspond to their stoichiometric coefficients, so for a reaction 2A + B ? A?B, the rate law is rate = k[A]²[B].

Effect of Reactant Concentration on Reaction Rate

Changing the concentration of reactants impacts the reaction rate based on the reaction order with respect to each reactant. In the rate law rate = k[A]²[B], doubling the concentration of A (which is second order) increases the rate by a factor of 4, while doubling the concentration of B (which is first order) increases the rate by a factor of 2.

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