The initial rate of a chemical reaction, P + Q Products , was measured at various initial concentrations of the reactants. The experimental data is provided in the accompanying table. Based on this data, which of the following represents the correct rate law for the reaction?

Step-by-step solution

Let the rate law be Rate = k[P]^x[Q]^y . From Experiment 1 and 2, when [Q] is kept constant at 0.02 mol L ⁻¹ , the concentration of [P] is increased from 0.02 to 0.06 (by a factor of 3 ). The rate increases from 4.0 10⁻⁵ to 1.2 10⁻⁴ (by a factor of 3 ). Rate ₂ Rate ₁ = k(0.06)^x(0.02)^y k(0.02)^x(0.02)^y 1.2 10⁻⁴ 4.0 10⁻⁵ = ( 0.06 0.02 )^x 3 = 3^x x = 1 From Experiment 2 and 3, when [P] is kept constant at 0.06 mol L ⁻¹ , the concentration of [Q] is increased from 0.02 to 0.04 (by a factor of 2 ). The rate increase