$t_{1/2} =$ constant confirms the first order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of reaction is ($a =$ initial concentration of reactant).

For a chemical reaction $A \to B$,it is found that the rate of reaction doubles when the concentration of $A$ is increased four times. The order of the reaction with respect to $A$ is:

The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

For the reaction $NO_2 + CO \rightarrow CO_2 + NO$,the rate law is given as $\text{Rate} = K [NO_2]^2$. What is the number of $CO$ molecules participating in the slow step?

Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

Write the unit of the rate constant for the following reactions:
$1.$ Zero order
$2.$ Second order