How do you solve first order half life reactions?

I'm studying for my chemistry midterm and I came across this problem and realized I do not have a clue how to do it? Can someone help me and show steps if possible. I know two equations that would be helpful, but I can't come up with the right answer. Equations I have been using are (half life= ln2/k) and ([A]=[A initial]e^-kt)

The half-life of the first order reaction, A → products, is 32.5 s. What was the original concentration, [A]O in mol/L, if after 2.2 minutes, the concentration of A is 0.0545 mol/L? Round your answer to three significant figures.

Correct Answer is .910
Asked Mar 07, 2013

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