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gte
Guest
so i did an experiment and i am trying to determine the rate law for the reaction between formic acid and bromine. so far i got the following.
Rate=k [Br]^1 [HCOOH]^y
Rate=k'[Bromine]^x where k'=k[HCOOH]^y .
i solved the following values, x=1, y=1.09 and k=.292 i have two [HCOOH] molarity values, and i have two k' values; which is how i figured out y and k, but now i am not sure how that fits into the original equations : Rate=k [Br]^x [HCOOH]^y
Rate=k'[Bromine]^x
can someone shed some light into this madness.. plz...
Rate=k [Br]^1 [HCOOH]^y
Rate=k'[Bromine]^x where k'=k[HCOOH]^y .
i solved the following values, x=1, y=1.09 and k=.292 i have two [HCOOH] molarity values, and i have two k' values; which is how i figured out y and k, but now i am not sure how that fits into the original equations : Rate=k [Br]^x [HCOOH]^y
Rate=k'[Bromine]^x
can someone shed some light into this madness.. plz...