$A$ reaction which is of first order with respect to reactant $A$,has a rate constant $6 \, min^{-1}$. If we start with $[A] = 0.5 \, mol \, L^{-1}$,when would $[A]$ reach the value of $0.05 \, mol \, L^{-1}$?

Consider a certain reaction $A \rightarrow \text{Products}$ with $k = 2.0 \times 10^{-2} \ s^{-1}$. Calculate the concentration of $A$ remaining after $100 \ s$ if the initial concentration of $A$ is $1.0 \ mol \ L^{-1}$.

For the reaction $A_{(g)} \rightarrow B_{(g)} + C_{(g)}$,the rate law is $R = k[A]$. At the start $(t = 0)$,the total pressure is $100 \ mm$ and after $t = 10 \ min$,the total pressure is $120 \ mm$. The rate constant $(min^{-1})$ is:

The following data were obtained during the first order thermal decomposition of a gas $A$ at constant volume:
$A_{(g)} \rightarrow 2 B_{(g)} + C_{(g)}$

$S.No.$	$Time/s$	$Total Pressure/(atm)$
$1.$	$0$	$0.1$
$2.$	$115$	$0.28$

The rate constant of the reaction is . . . . . . $\times 10^{-2} \ s^{-1}$ (nearest integer).

The integrated rate law equation for a first-order gas-phase reaction $A(g) \rightarrow B(g) + C(g)$ is given by (where $P_i$ is the initial pressure and $P_t$ is the total pressure at time $t$):

How much time is required for a first-order reaction to be $3/4$ complete?