Question

For the reaction, \[\ce{A + B -> Products}\], the rate becomes doubled on doubling the concentration of A but remains unchanged on doubling the concentration of B. What is the rate law?

Answer 1

Given reaction:

\[\ce{A + B −> Product}\]

Observations:

When [A] is doubled, the rate doubles → the reaction is first order with respect to A.

When [B] is doubled, the rate remains unchanged → the reaction is zero order with respect to B.

Rate law is given as 

Rate = k[A]

This means:

Order with respect to A = 1

Order with respect to B = 0

Overall order = 1 + 0 = 1