Question

Rate of reaction $A+B\to products$ is given below:

S.No.	[A] Mol/ lit.	[B] Mol/ lit.	Initial rate
$1$	$0.01$	$0.01$	$0.005$
$2$	$0.02$	$0.01$	$0.010$
$3$	$0.01$	$0.02$	$0.005$

Determine the order of reaction with respect to $A$ and $B$.

Answer 1

Let the rate law for the reaction is:

$R=k{\left[A\right]}^x{\left[B\right]}^y$

$k$=rate constant

As the rate is unaltered by change in the concentration of $B$ (from data 1 and 3)

Therefore $y=0$

and it gets double when $A$ is twiced (fromm data 1 and 2)

Therefore it is directly proportional to $\left[A\right]$

hence $x=1$

Thus $R=k{\left[A\right]}^1{\left[B\right]}^0$

orderof reaction with respect to $A$ is $1$ and w.r.t. $B$ is $0$.