Reaction A + B -> P. [B] is held nearly constant (large excess). [A] decays exponentially.
Why does [A] follow first-order behavior even though true rate law is rate = k[A][B]?
- A
Stoichiometry is 1:1
- B
First order with respect to time only
- C
B is a catalyst
- Dcheck_circle
[B] ≈ constant absorbs into k_obs
Explanation
With [B] ≈ [B]0 constant, rate = k[B]0[A] is effectively first order in A.