The following results have been obtained during the kinetic studies of the reaction:

2A + B C + D


Experiment



[A]/mol L-1



[B]/mol L-1



Initial rate of formation of D/mol L-1min-1



I



0.1



0.1



6.0 × 10-3



II



0.3



0.2



7.2 × 10-2



III



0.3



0.4



2.88 × 10-1



IV



0.4



0.1



2.40 × 10-2



Determine the Rate law and the rate constant for the reaction.


By comparing Experiment I and IV if we increase the concentration of A by 4 times then Rate also increased by 4 times. That means order with respect to A is 1.

By comparing Experiment II and III if we double the concentration of B Rate increases by 4 times that means order with respect to B is 2.


Rate law of reaction will be, Rate = k [A][B]2


To find K, K = rate/[A][B]2 i.e. K = 6.0 × 10-3/[0.1][0.1]2


K = 6 mol-2L2sec-1


Order with respect to A and B is 1 and 2 Respectively. And value of K(rate constant) is = 6 mol-2L2sec-1


11
1