Question

The· reaction, \[\ce{2A + B + C -> D + E}\], is found to be of first order in A, second order in B and zero order in C.

1. Give the rate law for the reaction in the form of a differential equation.
2. How is the rate affected on increasing the concentration of A, B and C two times?

Answer 1

i. The rate law of the given reaction is 

Rate = k [A] [B]² [C]⁰

or `(dx)/(dt) = k [A] [B]^2`

ii. Suppose the rate of reaction is r₁. Therefore,

r₁ = k [A] [B]²

When the concentrations of A, B and C are increased two times, suppose the new rate is r₂.

Therefore,

r₂ = k × {2 × [A]} × {2 × [B]}² × {2 × [C]}⁰

= 8 k [A] [B]²

= 8 r₁

Thus, the rate increases by 8 times.