The reaction
2A + B <--> C + D
is found to take place in two steps, the first, which follows second order kinetics is slow and the second is fast. Which of the following CANNOT be the mechanism for the rate determining step of this reaction?
A) A collides with B
B) A collides with A
C) B collides with B
D) 2 A collides with 1 B
I do not understand where they are getting the relationship between reaction order and the number of reactants. Can anyone shed some light?
2A + B <--> C + D
is found to take place in two steps, the first, which follows second order kinetics is slow and the second is fast. Which of the following CANNOT be the mechanism for the rate determining step of this reaction?
A) A collides with B
B) A collides with A
C) B collides with B
D) 2 A collides with 1 B
D) 2A collides with 1 B
The rate determining step follows second order kinetics. So, it must only involve two reactant molecules. Although it is often said the kinetics of a reaction cannot be derived from its stoichiometry, this is only true of the overall reaction. When a complex reaction is broken down to a series of elementary reactions, we can derive the rate law form slowest of elementary reactions.
D) has 3 reactant molecules so its wrong
The rate determining step follows second order kinetics. So, it must only involve two reactant molecules. Although it is often said the kinetics of a reaction cannot be derived from its stoichiometry, this is only true of the overall reaction. When a complex reaction is broken down to a series of elementary reactions, we can derive the rate law form slowest of elementary reactions.
D) has 3 reactant molecules so its wrong
I do not understand where they are getting the relationship between reaction order and the number of reactants. Can anyone shed some light?