The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor of:

The rate constant of a first order reaction at $27^{\circ} C$ is $10^{-3} \ min^{-1}$. The temperature coefficient of this reaction is $2$. What is the rate constant (in $min^{-1}$) at $17^{\circ} C$ for this reaction?

Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:

$[A_2]_0$	$[B_2]_0$	Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$	$0.1 \ M$	$2.5 \times 10^{-4}$
$0.2 \ M$	$0.1 \ M$	$5.0 \times 10^{-4}$
$0.2 \ M$	$0.2 \ M$	$1.0 \times 10^{-3}$

The value of the rate constant for the above reaction is:

For the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?

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

Which of the following is a bimolecular reaction?