Question

During Kinetic study of reaction 2A + B $\mapsto$ C + D, the following results were obtained: | A[M]| B[M]| initial rate of
formation of D
---|---|---|---
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

Based on above data, overall order of the reaction is ..........

Answer 1

From the rate law:
$r = k[A]^x[B]^y$
Using the data:
$\text{From (I) and (IV): } \frac{2.4 \times 10^{-2}}{6 \times 10^{-3}} = \frac{(0.4)^x}{(0.1)^x} \implies 4 = 4^x \implies x = 1$
$\text{From (III) and (II): } \frac{2.88 \times 10^{-1}}{7.2 \times 10^{-2}} = \frac{(0.4)^y}{(0.2)^y} \implies 4 = 2^y \implies y = 2$
Overall order = $x + y = 1 + 2 = 3$.