Chemistry - Chemical Kinetics Question with Solution | TestHub

$A⟶B$ Initial concentration Rate of reaction $$\begin{array}{ll}2\times 10^{-3}\mathrm{M}& 2.40\times 10^{-4}{\mathrm{Ms}}^{-1}\\ 1\times 10^{-3}\mathrm{M}& 0.60\times 10^{-4}{\mathrm{Ms}}^{-1}\end{array}$$ rate of reaction $$r=k[A{]}^x$$ where $x=$ order of reaction hence $$\begin{array}{rl}& 2.40\times 10^{-4}=k{\left[2\times 10^{-3}\right]}^x\\ & 0.60\times 10^{-4}=k{\left[1\times 10^{-3}\right]}^x\end{array}$$ on dividing eqn.(i) from eqn. (ii) we get $4=(2{)}^x$ $\therefore x=2$ i.e. order of reaction $=2$