Problem: The reaction A => B + C is second order in A. When the initial [A] = 0.100 M, the reaction is 20.0% complete in 26.2 minutes. Calculate the value of the rate constant (in L/min·mol).a. 8.22x10-2 b. 9.54x10-2c. 1.53d. 1.05e. 0.91

FREE Expert Solution

We’re being asked to determine the rate constant (k) of a second-order reaction:

 B + C


The concentration of A decreases by 80% (from 100% - 20% = 80%) starting 0.1 M in 26.2 minutes. 80% of 0.1 M is:


0.1 M x 0.8 = 0.08 M


The integrated rate law for a second-order reaction is as follows:


1[A]t=kt+1[A]0


where: 

[A]t = concentration at time t

k = rate constant

t = time

[A]0 = initial concentration


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Problem Details

The reaction A => B + C is second order in A. When the initial [A] = 0.100 M, the reaction is 20.0% complete in 26.2 minutes. Calculate the value of the rate constant (in L/min·mol).

a. 8.22x10-2 

b. 9.54x10-2

c. 1.53

d. 1.05

e. 0.91

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