NCERT Solutions for Chapter: Chemical Kinetics, Exercise 1: Intext Questions

For the reaction $\mathrm{R}\to \mathrm{P},$ the concentration of a reactant changes from $0.03 \mathrm{M}$ to $0.02 \mathrm{M}$ in $25$ minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

In a reaction, $2\mathrm{A}\to$ Products, the concentration of $\mathrm{A}$ decreases from $0.5 \mathrm{m}\mathrm{o}\mathrm{l} {\mathrm{L}}^{-1}$ to $0.4 \mathrm{m}\mathrm{o}\mathrm{l} {\mathrm{L}}^{-1}$ in $10$ minutes. Calculate the rate during this interval?

For a reaction, $\mathrm{A}+\mathrm{B}\to$ Product; the rate law is given by, $\mathrm{r}=\mathrm{k}{\left[\mathrm{A}\right]}^{\frac{1}{2}}{\left[\mathrm{B}\right]}^2.$ What is the order of the reaction?

The conversion of molecules $\mathrm{X}$ to $\mathrm{Y}$ follows second order kinetics. If concentration of $\mathrm{X}$ is increased to three times how will it affect the rate of formation of $\mathrm{Y}$?