Identify the order of reaction if its rate constant is $x \ sec^{-1}$.

For a chemical reaction,$2A + 2B \to C + D$,the order of reaction is $1$ with respect to $A$ and $1$ with respect to $B$. The initial rate of the reaction is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. When $50\%$ of the reactants are converted into products,the rate of the reaction would become:

For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:

Expt. no.	$[A]$	$[B]$	Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$	$0.2$	$0.2$	$2$
$2$	$0.2$	$0.4$	$4$
$3$	$0.6$	$0.4$	$36$

For a reaction,$K = 4.5 \times 10^{-4} \ L \ mol^{-1} \ s^{-1}$. What is the order of the reaction?

The unit of the rate constant for a second-order reaction is ....

Why can we not determine the order of a reaction by taking into consideration the balanced chemical equation?