Question

The half life of a first order reaction is 36.8 seconds. How many seconds must the reaction proceed before the reaction is 72.5% completed?

Answer 1

It would take approximately

64.0

s

given those data.

Step-by-step explanation:

21.3

s

=

0.693

k

∴

k

≈

3.25

⋅

10

−

2

s

−

1

ln

(

1

8

)

=

−

3.25

⋅

10

−

2

s

−

1

⋅

t

∴

t

≈

64.0

s

Each equation I used is assuming this reaction's kinetics are of the first order, which is cited. The first equation is a simplified version for the half life of a first order reactant, and the second equation is the general equation for first order reactions in chemical kinetics.