The rate constant of a reaction is $0.693 \times 10^{-2} \ min^{-1}$. What is the half-life period (in $s$)?

The decomposition of benzene diazonium chloride is a first order reaction. The time taken for the decomposition of $\frac{1}{4}$ and $\frac{1}{10}$ of its initial concentration are $t_{1/4}$ and $t_{1/10}$ respectively. The value of $\frac{t_{1/4}}{t_{1/10}} \times 100$ is (Given: $\log 2 = 0.3, \log 3 = 0.477$)

$A$ first order reaction is $50 \%$ completed in $16 \ minutes$. Find the percentage of reactant reacting in $32 \ minutes$. (in $\%$)

If the rate constant of a reaction is $x \, sec^{-1}$,by what factor does the rate increase if the initial concentration of $A$ is tripled?

For the reaction $2A + B \to \text{Product}$,the rate law is given as $\frac{-d[A]}{dt} = K[A]$. At a time when $t = \frac{1}{K}$,the concentration of the reactant $A$ is ($Co =$ initial concentration).

The rate constant and half-life of a first-order reaction are related to each other as -