Problem: The half-life of a reaction of compound A to give compounds D and E is 8.50 min when the initial concentration of A is 0.150 mol/L. How long will it take for the concentration to drop to 0.0300 mol/L if the reaction is(b) second order with respect to A?

FREE Expert Solution

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




Calculate k:

The half-life of a second-order reaction is given by:


t1/2=1k[A]0


where:

k = rate constant

[A]0 = initial concentration


t1/2=1k[A]0

8.50 min=1k(0.150 mols)

k=1(0.150 molL)(8.50 min) 


k = 0.7843 L/mol • min



Solving for time:


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

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Problem Details

The half-life of a reaction of compound A to give compounds D and E is 8.50 min when the initial concentration of A is 0.150 mol/L. How long will it take for the concentration to drop to 0.0300 mol/L if the reaction is

(b) second order with respect to A?

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