For the non-stoichiometric reaction 2A+B→C+D, the following kinetic data were obtained in three separate experiments, all at 298 K. Initial concentration of AInitial concentration of BInitial rate of formation of C in mol ⁡L−1s−10.1 M0.1 M1.2×10−3 0.1 M0.2M1.2×10−30.2M0.1 M2.4×10−3The rate law for the formation of C is

A
$d [C] / d t = k [A]$
B
$d [C] / d t = k [A] [B]$
C
$d [C] / d t = k [A]^{2} [B]$
D
$d [C] / d t = k [A] [B]^{2}$

Solution:

On changing the concentration of B to twice without changing the concentration of A, there is no change in the rate of reaction. Hence, the order of the reaction with respect to B is zero. On changing the concentration of A to twice without changing the concentration of B, the rate of reaction becomes twice. Hence, the order of the reaction with respect to A is one.

Initial concentration of A	Initial concentration of B	Initial rate of formation of C in $mol L^{- 1} s^{- 1}$
0.1 M	0.1 M	$1.2 \times 10^{- 3}$
0.1 M	0.2M	$1.2 \times 10^{- 3}$
0.2M	0.1 M	$2.4 \times 10^{- 3}$

Solution:

Related content