$75\%$ of a first order reaction is completed in $30 \ min$. What is the time required for $93.75\%$ of the reaction (in minutes)?

For a reaction,the rate constant is $2.34 \ s^{-1}$. The half-life period for the reaction is ....... $s.$

In a first order reaction,$60 \%$ of the reactant converts into product in $45 \ minutes$. Calculate the rate constant of the reaction.

Time required to decompose $SO_2Cl_2$ to half of its initial amount is $60 \ min$. If the decomposition is a first order reaction,calculate the rate constant of the reaction. (in $min^{-1}$)

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

For the decomposition of azomethane,$CH_3N_2CH_{3(g)} \rightarrow CH_3CH_{3(g)} + N_{2(g)}$,a first order reaction,the variation in partial pressure with time at $600 \ K$ is given as shown in the graph. The value of the rate constant $k$ in $s^{-1}$ is $x \times 10^4$. Find the value of $x$.