Question

Consider the following reaction: 2A + 3B 2C+D If the rate of reaction does not change when the concentration of B is doubled, we may say that: a. The reaction is first order with respect to B The reaction is zero order with respect to B c. The reaction is second order with respect to A d. The reaction is third order with respect to B

Answer 1

Answer:

The reaction is zero order with respect to B

Explanation:

The reaction given in the question is -

2A  + 3 B ---->  2C + D

From , the above reaction the rate law is written as -

rate = k [ A ]²[ B ]³

where ,

k = rate constant

In the above equation the order is determined by the sum of the powers of the concentrations , i.e. 2 + 3 = 5 order , which never possible ,

Hence , in the question ,

The by changing the concentration of B , the rate does not change .

hence , the rate is independent of the concentration of B .

Therefore ,

The order with respect to B will be zero .