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

Correct Answer: 3

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 = \(x + y = 1 + 2 = 3\).