Looking at the chemical reaction: [(H3C)2NC6H4]3C+ + OH- --> [(H3C)2NC6H4]3COH , is it reasonable for the crystal violet reaction to occur by a single step mechanism? Why, or why not?
Based on the rate law, rate = k[crystal violet+][OH-], could the crystal violet reaction occur by a single-step mechanism? Why or why not?
Thanks in advance!
To determine if the crystal violet reaction can occur by a single-step mechanism, we can analyze the reaction and the rate law provided.
First, let's examine the chemical reaction:
[(H3C)2NC6H4]3C+ + OH- --> [(H3C)2NC6H4]3COH
In this reaction, a cationic crystal violet molecule reacts with a hydroxide ion to form a neutral product.
Now, let's consider the rate law:
rate = k[crystal violet+][OH-]
The rate law indicates that the rate of the reaction depends on the concentrations of both the crystal violet cation and the hydroxide ion.
A single-step mechanism implies that the overall reaction occurs in a single step, where the reactants collide and form the product directly. In this case, if the rate law is consistent with a single-step mechanism, the exponents of the reactant concentrations in the rate law (here crystal violet+ and OH-) would correspond to the number of molecules participating in the rate-determining step.
In the given rate law, the rate is proportional to the concentration of both crystal violet+ and OH-. This suggests that both species are involved in the rate-determining step, supporting the idea that the reaction involves more than one step.
Furthermore, the fact that crystal violet+ and OH- are both included in the rate law suggests that they are reactants and not intermediates. If they were intermediates, they would appear in the mechanism but not in the rate law.
Therefore, based on the rate law and the dependence of the rate on the reactants' concentrations, it is reasonable to conclude that the crystal violet reaction likely occurs through a multi-step mechanism and not a single-step mechanism.