The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

The rate constant for a reaction is $10.8 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$. The order of the reaction is .......

If the decomposition of hydrogen peroxide is a first-order reaction,its rate law equation can be represented as:

The value of the rate constant of a pseudo first order reaction:

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.

The rate constant for a second order reaction,$A \rightarrow \text{Product}$ is $1.62 \ M^{-1} \ s^{-1}$. What will be the rate of reaction when concentration of reactant is $2 \times 10^{-3} \ M$ (in $M \ s^{-1}$)?