The order of the reaction occurring by following mechanism should be

$(i)$ ${A_2} \to A + A$ (fast)

$(ii)$ $A + {B_2} \to AB + B$ (slow)

$(iii)$ $A + B \to $ (fast)

Which of these does not influence the rate of reaction

In the following reaction $A \longrightarrow B + C$, rate constant is $0.001\, Ms^{-1}$. If we start with $1\, M$ of $A$ then concentration of $A$ and $B$ after $10\, minutes$ are respectively

For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways

$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ;    $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$

So the correct relation between $K$ and $K_1$ is

The order of a reaction is said to be $ 2 $ with respect to a reactant $X, $ when

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

For the reaction the rate of formation of $C$ will be