Mention True $(T)$ and False $(F)$ statements for the following expressions related to a zero-order reaction $R \to P$:
$I. \ k = \frac{[R]_0}{2 t_{1/2}}$
$II. \ t_{1/2} = \frac{[R]_0}{4k}$

In the reaction,$A + B \to C + D$,the rate $\left( \frac{dx}{dt} \right)$ when plotted against time $t$ gives a straight line parallel to the time axis. The order and rate of reaction will be

The half-life of a zero order reaction $A \rightarrow \text{products}$ is $0.5 \ hr$. The initial concentration of $A$ is $4 \ mol \ L^{-1}$. How much time (in $hr$) does it take for its concentration to come from $2.0 \ mol \ L^{-1}$ to $1.0 \ mol \ L^{-1}$?

For a zero-order reaction $A \rightarrow \text{Product}$,the half-life is $1 \ h$. If the initial concentration of reactant $A$ is $2.0 \ mol \ L^{-1}$,how many hours will it take for the concentration to decrease from $0.50 \ mol \ L^{-1}$ to $0.25 \ mol \ L^{-1}$?

For a zero order reaction,a plot of $t_{1/2}$ versus $[A]_0$ will be

For a zero-order reaction,the rate constant $K = 2 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,then its initial concentration must be ...... $M$.