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?

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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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Integrated Rate Law concept. You can view video lessons to learn Integrated Rate Law. Or if you need more Integrated Rate Law practice, you can also practice Integrated Rate Law practice problems.

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Based on our data, we think this problem is relevant for Professor Price's class at GVSU.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.