Half life of a first order reaction is $20 \ min$. The time taken to reduce the initial concentration of reactant to $(1/10)^{th}$ is $\qquad$ (in $min$)

The following data were obtained during the first order thermal decomposition of $N_{2}O_{5(g)}$ at constant volume:
$2N_{2}O_{5(g)} \rightarrow 2N_{2}O_{4(g)} + O_{2(g)}$

$S.No.$	Time $/$ $s$	Total pressure $/$ $atm$
$1.$	$0$	$0.5$
$2.$	$100$	$0.512$

Calculate the rate constant.

Rate of a first order reaction is $1.5 \times 10^{-2} \ mol \ L^{-1} \ minute^{-1}$ at $0.5 \ M$ concentration of reactant,calculate half life of reaction.

For an elementary reaction,$X_{(g)} \rightarrow Y_{(g)} + Z_{(g)}$,the $t_{1/2}$ is $10 \text{ minutes}$. In what period of time would the concentration of $X$ be reduced to $10 \%$ of its original concentration?

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 half-life of a first-order reaction is $20 \text{ minutes}$. What is the rate constant (in $\text{min}^{-1}$) for this reaction?