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

# For the non-stoichiometric reaction $2\mathrm{A}+\mathrm{B}\to \mathrm{C}+\mathrm{D}$, 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 0.1 M0.1 M$1.2×{10}^{-3}$ 0.1 M0.2M$1.2×{10}^{-3}$0.2M0.1 M$2.4×{10}^{-3}$The rate law for the formation of C is

1. A

$\mathrm{d}\left[\mathrm{C}\right]/\mathrm{d}t=k\left[\mathrm{A}\right]$

2. B

$\mathrm{d}\left[\mathrm{C}\right]/\mathrm{d}t=k\left[\mathrm{A}\right]\left[\mathrm{B}\right]$

3. C

$\mathrm{d}\left[\mathrm{C}\right]/\mathrm{d}t=k\left[\mathrm{A}{\right]}^{2}\left[\mathrm{B}\right]$

4. D

$\mathrm{d}\left[\mathrm{C}\right]/\mathrm{d}t=k\left[\mathrm{A}\right]\left[\mathrm{B}{\right]}^{2}$

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### 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.

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