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. 6.54x10-2B. 9.54x10-5C. 1.52D. 9.54x10-2E. 4.40

FREE Expert Solution

 We’re being asked to calculate the value of the rate constant (in L/min•mol) for the reaction below if the reaction is 20.0 =% complete in 26.2%


A → B + C


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 (unknown)

[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. 6.54x10-2
B. 9.54x10-5
C. 1.52
D. 9.54x10-2
E. 4.40

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