For a first-order reaction,the half-life period is $69.3 \ s$. If the concentration of the reactant is $0.10 \ mol \ L^{-1}$,what will be the rate of the reaction?

$A$ first order reaction was started with a decimolar solution of the reactant. $8$ minutes and $20$ seconds later,its concentration was found to be $M/100$. The rate constant of the reaction is:

The initial concentration of $N_2O_5$ in the following first order reaction $N_2O_{5(g)} \rightarrow 2NO_{2(g)} + 1/2O_{2(g)}$ was $1.24 \times 10^{-2} \, mol \, L^{-1}$ at $318 \, K$. The concentration of $N_2O_5$ after $60 \, minutes$ was $0.20 \times 10^{-2} \, mol \, L^{-1}$. Calculate the rate constant of the reaction at $318 \, K$.

If the concentration of a first order reaction is increased by $x$ times,then the rate constant $(k)$ becomes

Calculate the rate constant for the first order reaction,$A \rightarrow B$ if the rate of reaction is $5.4 \times 10^{-6} \ mol \ dm^{-3} \ s^{-1}$ and $[A]=0.3 \ M$.

For a first-order reaction,the rate constant is $4 \times 10^{-3} \, s^{-1}$. If the concentration of the reactant is $0.02 \, M$,what will be the rate of the reaction?