Answer:
The reaction is second order in A(g), first order in B(g) and zero order in C(g)
Step-by-step explanation:
A non elementary reaction is a reaction that does not take place in a single reactive encounter. This implies that the reaction occurs in steps as shown in the question above.
C(g) is an intermediate, hence it does not occur in the overall reaction equation. The overall reaction equation is: 2A(g) + B(g) ---> 2D(g)
The rate law of the rate determining step is obtained from;
Rate= k1[A] [B] for fast step
Rate= k2 [A] [C] for slow step
But rate of forward reaction = rate of reverse reaction
k1[A] [B] = k-1 [C]
But [C] =k1 [A] [B]/k-1
Hence
Substitute into
Rate = k2 [A] [C]
Rate = k2k-1[A]^2 [B]/k-1
But k2k-1/k = K
Hence;
Rate = K [A]^2 [B]