Question

After 62.0 min, 33.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?

Answer 1

for a first order reaction, the half life = (ln2)/k. In order to find half life, we need to find the rate constant, k
the equation for a first oreder reaction, ln[A] = ln[A]o -kt
at time t= 62 min, [A] = 67% [A]o or 0.67[A]o
Subs these value into the equation to find the k's value.
After getting the value of k then use the half life equation for first order to find the half life.