Question

A reaction is first order in A and second order in B.

(i) Write the differential rate equation.

(ii) How is the rate affected by increasing the concentration of B, three times, keeping the concentration of A constant?

(iii) How is the rate affected by when the concentration of both A and B are doubled?

Answer 1

(i) A + B → product
rate = k [A] [B]²

(ii) If the concentration of B is tripled, the rate increases by 9 times i.e.,

(iii) If the concentration of both A and B are doubled, the rate increases by 8 times.