Question

After 54.0 min, 34.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?

Answer 1

use this equation: \(\huge A_{t}=A_0*e^{\color{red}{-\frac{0.693t}{t_{1/2}}}}\)
where \(A_{t}\) is the amount after t time elapsed, \(A_0\) is the initial amount. t is time, \(t_{1/2}\) is half life.

ps"\(\Large {-\frac{0.693t}{t_{1/2}}}\)", the part in red, is all in the exponent.