A following mechanism has been proposed for a reaction
$$\eqalign{
& 2A + B \to D + E \cr
& A + B \to C + D\left( {{\text{slow}}} \right) \cr
& A + C \to E\left( {{\text{fast}}} \right) \cr} $$
The rate law expression for the reaction is :
A.
$$r = k{\left[ A \right]^2}\left[ B \right]$$
B.
$$r = k\left[ A \right]\left[ B \right]$$
C.
$$r = k{\left[ A \right]^2}$$
D.
$$r = k\left[ A \right]\left[ C \right]$$
Answer :
$$r = k\left[ A \right]\left[ B \right]$$
Solution :
From slow reaction
$${\text{Rate}} = k\left[ A \right]\left[ B \right]$$
Releted MCQ Question on Physical Chemistry >> Chemical Kinetics
Releted Question 1
If uranium (mass number 238 and atomic number 92) emits an $$\alpha $$ -particle, the product has mass no. and atomic no.