Question

After 55.0 min, 34.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?

Answer 1

Beginning amount = 100
Final amount = 100-41
Elapsed time = 55 min

I believe if I have it right:
\[half-life = \frac{ \log2(elapsed time) }{ \log(\frac{ {initial} }{ final }) }\]
\[final-amount = \frac{ initial }{ 2^n }\]
where \[n = \frac{ elapsed-time }{ half-life }\]