Discussion Forum



1)

 For the  non-stoichiometric reaction 2A+B→ C+D, the following kinetic data were obtained in three separate experiments, all at 298 K

1632021895_C1.JPG

  The rate law for the formation of C is 


A) $\frac{dC}{dt}= k[A]^{}[B]^{}$

B) $\frac{dC}{dt}= k[A]^{2}[B]^{}$

C) $\frac{dC}{dt}= k[A]^{}[B]^{2}$

D) $\frac{dC}{dt}= k[A]$

Answer:

Option D

Explanation:

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 

     $r=\frac{dC}{dt}=k[A]^{x}[B]^{y}$

  where x= order of reaction w.r.t A

        y= order of reaction w.r.t B

$1.2\times10^{-3}=k(0.1)^{x}(0.1)^{y}$

$1.2\times10^{-3}=k(0.1)^{x}(0.2)^{y}$

$2.4\times10^{-3}=k(0.2)^{x}(0.1)^{y}$

$R= k[A]^{1}[B]^{0}$

 As shown above, rate of reaction remains constant as the concentration of reactant (B)  changes from 0.1 M to 0.2 M  and becomes double when the concentration  of A change from 0.1 to 0.2  B(i.e doubled)