If the reaction between $A$ and $B$ to give $C$ shows first-order kinetics in $A$ and second-order in $B$,the rate equation can be written as:

Why is the probability of a reaction with molecularity higher than $3$ very rare?

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:

$[AB] \ (mol \ dm^{-3})$	Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$	$2.75 \times 10^{-8}$
$0.40$	$11.0 \times 10^{-8}$
$0.60$	$24.75 \times 10^{-8}$

The order for the decomposition of $AB$ is:

The rate constant of which of the following reactions is independent of the concentration of the reactants?

For an $n^{th}$ order reaction,the rate law is given by $\frac{dx}{dt} = K[A]^n$. Which parameter can be determined from the logarithmic plot?

The rate constant for the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$ is $3.0 \times 10^{-5} \text{ s}^{-1}$. If the rate of reaction is $2.4 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}$, then the concentration of $N_2O_5$ in $\text{mol L}^{-1}$ is: