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Test 3 #8

Posted: Wed Mar 14, 2018 12:18 am
by Kelly Kiremidjian 1C
8.) In a 2nd order reaction, a reactant has a known half-life of 3.00 minutes and an initial concentration of 5.00 M. How much time (in seconds) will it take for the concentration of this reactant to drop to 2.00 M?

Could someone explain how they did this question?

Re: Test 3 #8

Posted: Wed Mar 14, 2018 12:59 am
by Qining Jin 1F
Since you have the half life and initial concentration, you can solve for k using the equation for second order half-life

t(1/2) = 1/(k[A]naught)

After solving for k, you can use the second order equation

1/[A] = kt + 1/[A]naught

Plug in 2.00M for [A], 5.00M for [A]naught, and k
then solve for t

Re: Test 3 #8

Posted: Wed Mar 14, 2018 11:48 am
by RohanGupta1G
use the half life to solve for k and then use the integrated rate law.