In the following reaction $A \to B + C$,the rate constant is $0.001 \, M/sec$. If we start with $1 \, M$ of $A$,the concentrations of $A$ and $B$ after $10$ minutes are respectively:

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.

For a zero order reaction $A \rightarrow \text{product}$,a plot of $[A]$ (on $y$-axis) and time (on $x$-axis) gave a straight line with slope equal to $-3 \times 10^{-3} \ M \ min^{-1}$ and intercept equal to $2 \times 10^{-2} \ M$ (on $y$-axis). What is the rate constant (in $M \ min^{-1}$) of this reaction?

Which of the following equations represents the integrated rate law for a zero order reaction?

The rate constant of a zero-order reaction is $0.2 \ mol \ L^{-1} \ hr^{-1}$. If the concentration of the reactant after $0.5 \ hr$ is $0.05 \ M$,then the initial concentration of the reactant is ....... $M$.

Which among the following reactions is an example of a zero-order reaction?