In: Chemistry
The overall reactions and rate laws for several reactions are given below. Which one of these represents an elementary step?
A) A + 2B → P rate = k[A]2
B) A + 2B → P rate = k[A][B]
c) 2A → P rate = k[A]
D)A + B + C → P rate = k[A][C]
E) A + B → P rate = k[A][B]
If the rate law can be derived from the given reaction, then the given reaction can be said to be elementary reaction
E is elementary reaction because rate law from reaction will be
rate = k [A] [B]
which is same as given rate law
Answer: E
for A, rate law from given reaction is
rate= k [A] [B]^2 which do not match given rate law
for B, rate law from given reaction is
rate= k [A] [B]^2 which do not match given rate law
for C, rate law from given reaction is
rate= k [A]^2 which do not match given rate law
for D, rate law from given reaction is
rate= k [A] [B] [C] which do not match given rate law