The time required for completion of $$93.75 \%$$ of a first order reaction is $$x$$ minutes. The half-life of it (in minutes) is

. The rate constant for a zero order reaction $$A \longrightarrow$$ products is $$0.0030 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~S}^{-1}$$. How long it will take for the initial concentration of $$A$$ to fall from 0.10 M to 0.075 M ?

For a $$A+B \rightarrow$$ products, the rate of the reaction is given by rate $$=k[A][B]^2$$. The units of rate constant $$(k)$$ will be

For an elementary reaction, $$X(g) \longrightarrow Y(g)+Z(g)$$, the $$t_{1 / 2}$$ is $$10 \mathrm{~min}$$. In what period of time would the concentration of $$X$$ be reduced to $$10 \%$$ of its original concentration?