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

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 .

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