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