The half life of radioactive material is 24.1days. How long will a sample take to decay 90% of it
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half life period = 0.693/k
24.1 = 0.693/k
k = 0.693/24.1
k = 0.028755
All radioactive decays follow first order kinetics
kt = 2.303*log(100/10)
kt = 2.303
t =2.303/k
t = 2.303/0.028755
t = 80 days
24.1 = 0.693/k
k = 0.693/24.1
k = 0.028755
All radioactive decays follow first order kinetics
kt = 2.303*log(100/10)
kt = 2.303
t =2.303/k
t = 2.303/0.028755
t = 80 days
Answered by
1
Explanation:
It is given:
Charcoal has the initial activity, which is denoted as A_{0}=15.3A
0
=15.3 disintegrations per minute per gram.
Charcoal has the half-life, T 12=5730T12=5730 years
After a few years, the charcoal’s final activity, A = 12.3 disintegrations per minute per gram
Constant of disintegration,
\lambda=0.693 \mathrm{T} 12=0.6935370 \mathrm{y}-1λ=0.693T12=0.6935370y−1
For the action to attain 12.3 disintegrations per minute per gram, let the time taken by the sample at a time of t year.
Sample’s activity,
A=A O e-\lambda tA=AOe−λt
A=A O e-0.6935730 \times tA=AOe−0.6935730×t
\Rightarrow \mathrm{t}=1804.3 \text { years }⇒t=1804.3 years
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