If the rate constant $(K)$ of a reaction is $1.6 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$,the order of reaction is

The plot of concentration of a reactant versus time for a chemical reaction is shown below. The order of this reaction with respect to the reactant is

The rate constant for a zero order reaction $A \rightarrow$ products is $0.0030 \ mol \ L^{-1} \ s^{-1}$. How long will it take for the initial concentration of $A$ to fall from $0.10 \ M$ to $0.075 \ M$ (in $s$)?

The time for the half-life period of a certain reaction $A \rightarrow \text{Products}$ is $1 \ hr$. When the initial concentration of the reactant $A$ is $2.0 \ mol \ L^{-1}$,how many hours does it take for its concentration to decrease from $0.50 \ mol \ L^{-1}$ to $0.25 \ mol \ L^{-1}$ if it is a zero-order reaction?

Which of the following is the incorrect equation for the rate constant of a zero-order reaction?

What is the value of the slope of a graph obtained by plotting the concentration of reactant $[A]_t$ versus time for a zero order reaction?