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

For a reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $2$ and with respect to $B$ is $3$. If the concentration of both is doubled,by how much will the rate increase?

If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order:

Considering the reaction $aG + bH \rightarrow \text{Products}$,when the concentrations of both reactants $G$ and $H$ are doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled while the concentration of $H$ remains constant,the rate doubles. What is the overall order of the reaction?

For an elementary chemical reaction,$A_2 \underset{k_{-1}}{\overset{k_1}{\longleftrightarrow}} 2A$,the expression for $\frac{d[A]}{dt}$ is

What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$