For a reaction A + B Products , the following initial rate data were obtained: Experiment [A] (mol L ⁻¹ ) [B] (mol L ⁻¹ ) Initial Rate 1 0.1 0.1 R 2 0.2 0.1 2R 3 0.1 0.2 4R What will be the initial rate of the reaction when [ A ] = 0.2 mol L ⁻¹ and [ B ] = 0.2 mol L ⁻¹ ?

Step-by-step solution

Let the rate law be Rate = k[ A ]^x[ B ]^y . From Experiment 1 and 2, keeping [ B ] constant, doubling [ A ] (from 0.1 to 0.2 ) doubles the rate (from R to 2R ). Therefore, the reaction is first order with respect to A ( x = 1 ). From Experiment 1 and 3, keeping [ A ] constant, doubling [ B ] (from 0.1 to 0.2 ) quadruples the rate (from R to 4R ). Therefore, the reaction is second order with respect to B ( y = 2 ). The rate law is Rate = k[ A ][ B ]^2 . When [ A ] = 0.2 mol L ⁻¹ and [ B ] = 0.2 mol L ⁻¹ , both conc