The rate constant of the reaction $A \rightarrow B$ is $0.6 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}.$ If the concentration of $A$ is $5 \, M,$ then the concentration of $B$ after $20$ minutes is ......... $M.$

Which of the following statements is true?

For the reaction,$A \rightarrow$ products,if the graph of $[A]$ vs time gives a straight line,predict the order of the reaction.

When the initial concentration of the reactant is doubled,the half-life period of a zero order reaction:

The rate constant,$k$ of a zero order reaction $2 NH_{3(g)} \xrightarrow[1130 \ K]{Pt} N_{2(g)} + 3 H_{2(g)}$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is

For a reaction of $n^{th}$ order,the plot of $t_{1/2}$ versus initial concentration $[A]_0$ is a straight line. When the initial concentration is $2 \ mol \ L^{-1}$,the reaction takes $10 \ min$ to complete $50\%$. If the reaction takes $t \ min$ to complete $50\%$ when the initial concentration is $4 \ mol \ L^{-1}$,find $n$ and $t$ respectively.