Question

the order of reaction with respect to A and B are

Answer 1

A + B -- > product

the rate of the reaction is given as

R = k [ A ]^n [ B ] ^ m

here ,

• R = rate of the reaction
• k = rate constant
• [ A ] and [ B ] = conc of the reactant

Let the order of [ A ] and [ B ] be n and m respectively

we need to find the values of m and n

As per the question ,

the rate of the reaction was doubled when concentration of a was doubled

R ' = k [2 A ]^n [ B ] ^ m

R ' = 2 k [ A ]^n [ B ] ^ m

Now substituting k [ A ]^n [ B ] ^ m as R ,

R ' = 2 R

this means that the order of A must be 1

Therefore , n = 1

Now ,

the again the rate of the reaction was doubled when the concentrations of A and B both were doubled

R " = k [2 A ]¹ [ 2 B ] ^ m

from this we can conclude that the order of B must be zero

m = 0

R " = k [ 2 A ]¹ [2 B ] ^0

R " = k [ 2 A ]¹ × 1

R " = 2 R

ANSWER :

• n = 1 ,m = 0
• R = k [ A ]^1 [ B ] ^0