If $50\%$ of a reaction occurs in $100 \ s$ and $75\%$ of the reaction occurs in $200 \ s$,the order of this reaction is

What is the rate constant of a first-order reaction if $0.08 \ mol$ of reactant reduces to $0.02 \ mol$ in $23.03 \ min$ (in $min^{-1}$)?

The integrated rate equation is $Rt = \log C_0 - \log C_t$. The straight line graph is obtained by plotting

The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time will it take to reduce the concentration of the reactant to $1/20^{th}$ of its initial value (in $\text{ s}$)?

In a first order reaction,the concentration of the reactant is reduced to $(1/8)^{th}$ of its initial concentration in $23.03 \ min$. What is the half-life period of the reaction (in $min$)?

If a $99\%$ first-order reaction is completed in $32$ minutes,how many minutes will it take for $99.9\%$ of the reaction to be completed?