1. reaction rate laws are frequently used to investigate reaction mechanisms. wo
ID: 1018198 • Letter: 1
Question
1. reaction rate laws are frequently used to investigate reaction mechanisms. would your results to this experiment be consistent with either or both of the following mechanisms? a. single step bimolecular reaction between dye and NaClO b. slow unimolecular decomposition of the dye followed by a rapid electron transfer reaction with ClO- ion which mechanism is correct? can you be certain that a mechanism is correct?
I know the answer is the single step bimolecular reaction between dye and naclo. However I have a hard time explaining it. Can someone clarify what single step bimolecular reactions are and what they require in order to occur?
Explanation / Answer
A bimolecular reaction involves the collision of two particles. Bimolecular reactions are common in organic reactions such as nucleophilic substitution. The rate of reaction depends on the product of the concentrations of both species involved, which makes bimolecular reactions second-order reactions.
in experiment we determined the rate that bleach, an aqueous solution of sodium hypochlorite(NaClO) will oxidize a colored food dye. the rate law= - change in dye/ change in t
the rate law= k[Dye]^a[ClO]^b
NaOCl + Fast Green FCF -----> Colorless products
NaOCl + FD&C Red ------> Colorless products
The rate law for reaction
Rate =k[NaOCl]x [Green]y
Rate =k[NaOCl]u [Red]v
answer is a. single step bimolecular reaction between dye and NaClO
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