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### 7B.13

Posted: **Wed Mar 11, 2020 9:23 pm**

by **Ellis Song 4I**

The half-life of A in a second-order reaction is 50.5 s when [A]0 = 0.84 mol/L. Calculate the time needed for the concentration of A to decrease to (a) one-sixteenth (b) one-fourth; (c) one-fifth of its original value.

Can someone please explain this problem

### Re: 7B.13

Posted: **Wed Mar 11, 2020 9:30 pm**

by **Brooke Yasuda 2J**

One way you could do this problem is by using the equation for a second order half life reaction and calculating the K value. With this you can then use the integrated rate law for a second order reaction to find the time needed to reach the concentration that is being asked.

### Re: 7B.13

Posted: **Wed Mar 11, 2020 10:29 pm**

by **Long Luong 2H**

What I did was find k using the second order half-life equation. Following that, I divided the original original concentration by 16, 4, and 5 for a), b), and c). With both initial and final concentrations and k, I plugged those values into the second order integrated rate law equation to find t.