For a zero order reaction,which of the following statements is false?

Identify the following statements as True $(T)$ or False $(F)$ for a zero-order reaction $R \to P$:
$(i) \ d[R] = -k dt$
$(ii) \ d[R] = +k dt$

The order of reaction for which the units of rate constant are $mol \ dm^{-3} \ s^{-1}$ 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 half life $(t_{1/2})$ and completion time $(T)$ for a zero order reaction if $K = 0.001 \, mol \, L^{-1} \, sec^{-1}$ and initial concentration $(a) = 1 \, M$.

$A \rightarrow P$ 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 $10 \ s$?