If the rate of the reaction is equal to the rate constant,the order of the reaction is

The reaction $2A \rightarrow B + C$ follows zero-order kinetics when:

Which of the following is correct with respect to the graph given?
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$

For a reaction of $n^{th}$ order,the plot of $t_{1/2}$ versus initial concentration $[A]_0$ is a straight line. When the initial concentration is $2 \ mol \ L^{-1}$,the reaction takes $10 \ min$ to complete $50\%$. If the reaction takes $t \ min$ to complete $50\%$ when the initial concentration is $4 \ mol \ L^{-1}$,find $n$ and $t$ respectively.

Which of the following is a zero order reaction?

For a reaction,doubling the concentration of the reactant doubles the half-life period. What is the order of the reaction?