Question

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

Write the differential rate equation.

How is the rate affected on increasing the concentration of B three times?

How is the rate affected when the concentrations of both A and B are doubled?

Answer 1

Rate $=k\left[A\right][B{]}^2$

Rate $=k\left[A\right][3B{]}^2=9k[A\left]\right[B{]}^2$ Rate of reaction becomes 9 times

Rate $=k\left[2A\right][2B{]}^2=8k[A\left]\right[B{]}^2$ Rate of reaction becomes 8 times.