A reaction is first order in A and second order in B. How is the rate affected when the concentrations of both A and B are doubled?

Advertisement Remove all ads

#### Solution

When the concentrations of both A and B are doubled,

`-(d[R])/dt = k [A][B]^2`

`= k[2A][2B]^2`

`=8.k[A][B]^2`

Therefore, the rate of reaction will increase 8 times.

Concept: Integrated Rate Equations - First Order Reactions

Is there an error in this question or solution?

Advertisement Remove all ads

#### APPEARS IN

Advertisement Remove all ads

Advertisement Remove all ads