Question

12. Consider the data taken in lab for the following reaction. Given the slopes of tangent lines for two data points, solve for the reaction rate constant for the following reaction. AB → AB 046 Rate of Change of (AB) 062 036 014 [AB] When (AB) = 0.302. AAB)-267 x 10 st 02 024 022 016 0.14 012 When (AB) = 0.149, [AB]= 6.51 x 10 00 000 004 > so 75 100 125 150 175 200 225 230 275 25 50 750 550 550025 Time (s)

Answer 1

First we determine the order of reaction :
Rate 2/ rate 1 = k [AB]₁^n / k [AB]₂^n

form curve :

Rate 2/ rate 1 = 4.10 = k [0.302]^n / k [0.149]^n

2.03 ^n = 4.10

====> n = 2

thus, order of reaction = 2

rate = k [AB]²

from 1st data set :

2.67*10^-3 M/s = k [0.302 M]^2

k = 0.0293 M-1 sec-1