For a certain reaction $R \to \text{Product}$, the plot of concentration $[R]$ vs time has a negative slope as shown. The order of reaction is:

For a reaction $A \rightarrow$ products,the half-life period is $1 \ h$. The initial concentration of reactant $A$ is $2 \ M$. If this reaction is of zero order,how many hours will it take for the concentration of the reactant to decrease from $0.5 \ M$ to $0.25 \ M$?

$A \rightarrow P$ is a zero order reaction. At $298 \ K$ the rate constant of the reaction is $1 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. Initial concentration of '$A$' is $0.1 \ mol \ L^{-1}$. What is the concentration of '$A$' after $10 \ s$?

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

In the reaction,$A \rightarrow$ products,if the concentration of the reactant is doubled,the rate of the reaction remains unchanged. The order of the reaction with respect to $A$ is

For a certain reaction,$10\%$ of the reactant dissociates in $1 \ hour$,$20\%$ of the reactant dissociates in $2 \ hour$,and $30\%$ of the reactant dissociates in $3 \ hour$. What are the units of the rate constant?