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

Time required for $100\%$ completion of a zero order reaction is

Consider the reaction $aX \to bY$,for which the rate constant at $30^\circ C$ is $1 \times 10^{-3} \text{ mol L}^{-1} \text{ s}^{-1}$. Which of the following statements are true?
$A$. When concentration of $X$ is increased to four times,the rate of reaction becomes $16$ times.
$B$. The reaction is a second order reaction.
$C$. The half-life period is independent of the concentration of $X$.
$D$. Decomposition of $N_2O_5$ is an example of the above reaction.
$E$. $\ln \frac{[R]_0}{[R]}$ vs time is valid for the above reaction.

Calculate the rate constant of a zero order reaction if it is $90 \%$ completed in $90 \ s$.

What is the half-life time of a reaction? Derive the equation of half-life time $(t_{1/2})$ for a zero-order reaction.

At $T \ K$,if the rate constant for a zero order reaction is $2.5 \times 10^{-3} \ M \ s^{-1}$,the time required for the initial concentration of reactant $R$ to fall from $0.10 \ M$ to $0.075 \ M$ at the same temperature in seconds is: