A certain reaction has a fixed half-life of 125 sec, how much time does it take for 25.0% of the original reactant to be reacted?
Given that reaction has a fixed half-life of 125 sec.
That means, half life is independent on initial concentration.
Hence, it is a first order reaction.
For first order reaction,
half life t1/2 = 0.693 /k where k is rate constant
k = 0.693/ t1/2 --- Eq (1)
k = 1/t ln { [A]o/[A]t} ----- Eq (2)
From Eqs (1) and (2),
0.693/ t1/2 = (1/t) ln {[A]o/ [A]t} ------Eq (3)
Given that
half life t1/2 = 125 sec
time t = ?
Initial amount = 100 %
Final amount [A]t = 100 % - 25 % = 75 %
Substitute all the values in Eq (3),
0.693/ t1/2 = (1/t) ln {[A]o/ [A]t}
0.693/ 125 = (1/t) ln {100 %/ 75%}
t = (125/0.693) x ln {100 %/ 75%}
= 51.9 sec
t = 51.9 sec
Therefore,
it take 51.9 sec for 25.0% of the original reactant to be reacted.
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