For the decomposition reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$,the reaction follows first-order kinetics. Which of the following is true?

The rate of a first-order reaction is $0.04 \ mol \ L^{-1} \ s^{-1}$ at $10 \ s$ and $0.03 \ mol \ L^{-1} \ s^{-1}$ at $20 \ s$ after the initiation of the reaction. The half-life period of the reaction is ......... $s$. (in $.1$)

Half-life period of a first order reaction is $1386 \ s$. The specific rate constant of the reaction is

The half-life period of a first-order reaction is $138.6 \ min$. The rate constant of the reaction is: (in $min^{-1}$)

If the rate constant of a reaction is $0.03 \ s^{-1}$,how much time does it take for $7.2 \ mol \ L^{-1}$ concentration of the reactant to get reduced to $0.9 \ mol \ L^{-1}$ (in $s$)? (Given: $\log 2 = 0.301$)

The rate constant for a first order reaction is $7.0 \times 10^{-4} \ s^{-1}$. If initial concentration of the reactant is $0.080 \ M$,what is the half-life of the reaction?