For the reaction, $A + B \rightarrow P$, the rate law is rate $= k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1$ M, $[B] = 0.2$ M at $25^\circ$C. Calculate the rate constant of the reaction at the same temperature.

In first order reaction, 20 % concentration remains after 10 min. What would be the rate constant of reaction if $\log_{10}(5) = 0.6989$?

Identify a type of order of reaction that its unit of rate constant is mol dm$^{-3}$s$^{-1}$ from the following.

Identify the dimensional nature of nanoparticles by the following.