During the kinetic study of the reaction, 2 ~A + B C + D , following results were obtained: array |c|c|c|c| Run & [ A ] / mol L ⁻¹ & [ ~B ] / mol L ⁻¹ & array l Initial rate of formation of D / mol L ⁻¹ ~min ⁻¹ array I & 0.1 & 0.1 & 6.0 10⁻¹ II & 0.3 & 0.2 & 7.2 10⁻¹ III & 0.3 & 0.4 & 28.8 10⁻¹ IV & 0.4 & 0.1 & 24.0 10⁻¹ array Based on the above data which one of the following is correct?

Step-by-step solution

In case of (II) and (III) Keeping concentration of [A] constant, when the concentration of [ B ] is doubled, the rate quadruples. Hence it is second order with respect to B . In case of I & IV Keeping the concentration of [B] constant, when the concentration of [ A ] is increased four times, rate also increases four times. Hence, the order with respect to A is one. Hence Rate =k[ ~A ][ B ]²