Posted by Sara on Friday, June 28, 2013 at 4:30pm.
The halflife for the secondorder reaction of a substance A is 58.2 s when A0 = 0.63 mol L1 Calculate the time needed for the concentration of A to decrease to the following values.
(a) onethird of its original value
(b) onesixth of its original value
(c) oneseventh of its original value

Chemistry  DrBob222, Friday, June 28, 2013 at 6:06pm
What's wrong with substituting values into the second order equation and solving for time.
Could it be you don't know how to handle 1/3, 1/6, 1/7 th values?
If Ao = 0.63 then 1/3 that = ? for a; 1/6 that for b and 1/7 that for c.

Chemistry  Sara, Friday, June 28, 2013 at 6:22pm
I don't understand how to figure out K.
I used the information in the problem given to solve for k, and then plug that k in to solve for t, but it's not the correct answer.

Chemistry  DrBob222, Friday, June 28, 2013 at 6:45pm
t_{1/2} = [1/k(Ao)]

Chemistry  Sara, Friday, June 28, 2013 at 6:48pm
I understand, but what is K or how can I determine K?

Chemistry  DrBob222, Friday, June 28, 2013 at 8:08pm
The problem GIVES you the half life. Use that and the equation I provided above to determine k.
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