Given :
C + D → Products OR xC + yD → Products
(i) When the concentration of C is doubled,
The rate of the reaction increases by 4.
[C]2(final) = 2[C]1(initial) then R2(final) = 4R1(initial)
(In this, the concentration of D is assumed to be constant.)
Hence,
The reaction is second order in C.
∴ nc = 2
(ii) When the concentration of D is tripled,
Rate is tripled.
The concentration of C is assumed to be constant.
Hence,
The reaction is first order in D.
Rate law : Rate = A[C]2[D]
∴ (i) Order of the reaction = 3
(ii) Rate law : Rate = A[C]2[D]
