Chemical Kinetics - Result Question 20

####23. For the non-stoichiometric reaction, $2 A+B \rightarrow C+D$, the following kinetic data were obtained in three separate experiments, all at $298 K$.

(2014 Main)

Initial
concentration
$[A]$
Initial
concentration
$[B]$
Initial rate of
formation of $\boldsymbol{C}$
$\left(mol L^{-1} s^{-1}\right)$
(i) $0.1 M$ $0.1 M$ $1.2 \times 10^{-3}$
(ii) $0.1 M$ $0.2 M$ $1.2 \times 10^{-3}$
(iii) $0.2 M$ $0.1 M$ $2.4 \times 10^{-3}$

The rate law for the formation of $C$ is

(a) $\frac{d C}{d t}=k[A][B]$

(b) $\frac{d C}{d t}=k[A]^{2}[B]$

(c) $\frac{d C}{d t}=k[A][B]^{2}$

(d) $\frac{d C}{d t}=k[A]$

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Answer:

Correct Answer: 23. (d)

Solution:

  1. This problem can be solved by determining the order of reaction w.r.t. each reactant and then writing rate law equation of the given equation accordingly as

$$ R=\frac{d C}{d t}=k[A]^{x}[B]^{y} $$

where, $x=$ order of reaction w.r.t $A$

$$ y=\text { order of reaction w.r.t } B $$

$$ \begin{aligned}



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