1/2 life question?
The half-life for the first-order decomposition of A is 355 s. How much time must elapse for the concentration of A to decrease to:
a) one-fourth (Ans. 711 s
b) 15% of its original value (Ans. 9.7 x 102s)
c) One-ninth of its initial concentration? (Ans. 1126 s)
回答 (3)
a)
Let n be the number of half-lives.
(1/2)ⁿ = (1/4)
(1/2)ⁿ = (1/2)²
Hence, n = 2
Time taken = (355 s) × 2 = 711 s
====
b)
Let m be the number of half-lives.
(1/2)ᵐ = 15%
log(0.5ᵐ) = log(0.15)
m log(0.5) = log(0.15)
m = log(0.15)/log(0.5)
Time taken = (355 s) × [log(0.15)/log(0.5)] = 970 s
====
c)
Let k be the number of half-lives.
(1/2)ᵏ = 1/9
log(0.5ᵏ) = log(1/9)
k log(0.5) = log(1/9)
k = log(1/9)/log(0.5)
Time taken = (355 s) × [log(1/9)/log(0.5)] = 1125 s
in general
.. At = Ao * (1/2)^(t / half life)
where
.. At = amount remaining after time = t has elapsed
.. Ao = initial amount
.. t = elapsed time
and you can eyeball some of this and say
.. half lives.. .. . .amount remaining
.. . .. 0.. .. .. .. .. .. . .. 1
. .. ...1. .. .. .. .. . .....1/2
.. . ...2. . .. .. ... .. ... 1/4
.. .. ..3.. .. .. .. .. . ....1/8
each time a half life has passed, the amount remaining is cut in half
********
(a).. 2 half lives have passed.... t = ?
(b).. At = 0.15 * Ao -----> t = -log(0.15)/log(2) * half life = ?
(c).. (1/9) = (1/2)^(t / half life) --> t = log(9)/log(2) * half life = ?
YOU get to finish
For A 1st order reaction
rate constant, k= 0.683/t^(1/2)
given, Half-LIFE, t^(1/2)=355s
:. k= 0.693/355s = 1.95 x 10^(-3) s^(-1)
a) For A 1st order reaction
ln[A] =ln[A]o - kt
[A]= [A]o/4
ln( [A]o/4)= ln[A]o - 1.95 x 10^(-3) s^(-1)
t=711s
b) [A]o = 100, [A]=15
t=973s
c) [A]o =1 [A]= [A]0/9
ln( [A]o/9) =ln( [A]o) - 1.95 x 10^(-3) s^(-1)
t=1126s
收錄日期: 2021-04-18 18:33:52
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