Suppose the half$-$life is $48\mathrm{.}1s$ for a first order reaction and the reactant concentration is $0\mathrm{.}0631M57\mathrm{.}1s$ after the reaction starts. How many seconds after the start of the reaction does it take for the reactant concentration to decrease to $0\mathrm{.}0158M?$

Answer:

What is the rate when $[A]=0\mathrm{.}085M$ and $[B]=0\mathrm{.}056M?$

Hint given in feedback

Answer:

Use the rate equation for the correct order with the $k$ that you determined.

For the reaction: $3Br{O}_{(aq)}-cdotsBr{O}_3(aq)+2Br(aq)$

$[Br{O}^{-}$