For a chemical reaction $A \rightarrow B$,the rate of the reaction is $2 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$,when the initial concentration is $0.05 \ mol \ dm^{-3}$. The rate of the same reaction is $1.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ when the initial concentration is $0.1 \ mol \ dm^{-3}$. The order of the reaction is

The half-life for a second-order reaction is $30 \ min$. If the initial concentration is $0.1 \ M$,then the value of the rate constant will be $............ \ M^{-1} \ min^{-1}$.

The following reactions occur for the reaction of $NO$ with $Br_2$ to form $NOBr$:
$NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons NOBr_{2_{(g)}}$
$NOBr_{2_{(g)}} + NO_{(g)} \rightarrow 2 NOBr_{(g)}$
If the second reaction is the rate-determining step,the order of the reaction with respect to $NO_{(g)}$ will be:

The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

The reaction of formation of phosgene from $CO$ and $Cl_2$ is $CO + Cl_2 \to COCl_2.$ The proposed mechanism is
$(i)$ $Cl_2 \,\underset{k_2}{\overset{k_1}{\longleftrightarrow}}\, 2Cl$
$(ii)$ $Cl + CO \,\underset{k_4}{\overset{k_3}{\longleftrightarrow}}\, COCl$
$(iii)$ $COCl + Cl_2 \xrightarrow{k_5} COCl_2 + Cl$ (slow)
Find the correct expression of rate law.

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?