A certain reaction has the following general form.

$xAyB$

Concentration versus time data were collected for this reaction, and a plot of $ln[A]$ versus time$($sec$)$ resulted in a straight line of $y=-0\mathrm{.}0297x-3\mathrm{.}91.$

Determine

the rate law,

the value of the rate constant $(k)$ and

$3$ the initial concentration for this reaction.

How much time is required for the concentration of $A$ to decrease to $2\mathrm{.}50{10}^{-3}M?$

What is the concentration of A after $825$ seconds?