The following results were obtained during kinetic studies of the reaction. 2 A + B → product Experiment A in mol L - 1 B i n m o l L - 1 Initial rate of reaction in mol L - 1 min - 1 I 0 . 10 0 . 20 6.93 × 10 - 3 II 0 . 10 0 . 25 6.93 × 10 - 3 III 0 . 20 0 . 30 1.386 × 10 - 2 The time (in minutes) required to consume half of A is

Step-by-step solution

Let's assume x and y are the order of the reaction with respect to A and B , respectively. From equation 1 and 2 , 0 .1 0 .1 x 0 .2 0 .25 y = 6 .93 × 10 - 3 6 .93 × 10 - 3 ⇒ y = 0 From equation 1 and 3 and put the value y = 0 , 0 .1 0 .2 x 0 .2 0 .3 0 = 6 .93 × 10 - 3 1 .386 × 10 - 2 ∴ y = 0 1 2 x = 1 2 ⇒ x = 1 The rate law will be R = K [ A ] 1 [ B ] 0 Hence, the reaction is of the first order. K = R A = 6 .93 × 10 - 3 0 .1 = 6 .93 × 10 - 2 Here t 1 2 for the fir