91Ó°ÊÓ

• Mass of the charcoal sample, m = 5g
• Activity of the ${}^{14}C$nuclide of the charcoal sample, $R=(63\mathrm{disintergrations}/\min )per5.00g$
• Activity of the ${}^{14}C$nuclide of a living tree,$R_0=\left(15.3\mathrm{disintegrations}/\min \right)\mathrm{per}1.00\mathrm{g}$
• Mass of the living tree,${\mathrm{m}}_{\mathrm{tree}}=1.00\mathrm{g}$
• Half-life of ${}^{14}C$,$T_{1/2}=5730y$

The activity of the sample is the disintegrations of the sample per second. The exponential relation of the activity of the sample with the disintegration constant and time gives the required time value of the decaying charcoal.

Formulae:

The rate of undecayed sample after a given time, $R=R_0{e}^{-\mathrm{λ}t}……..\left(1\right)$

The disintegration constant, $\mathrm{λ}=\frac{\ln 2}{T_{1/2}}.........\left(2\right)$

where, $T_{1/2}$is the half-life of the substance.

Substituting equation (2) in equation (1) with the given data, the age of the charcoal can be given as follows:

$$\begin{gathered} t=\frac{1}{\mathrm{λ}}\ln \left(\frac{R_0}{R}\right) \\ =\left(\frac{T_{1/2}}{\ln 2}\right)\ln \left(\frac{R_0}{R}\right) \\ =\left(\frac{5730y}{\ln 2}\right)\ln \left(\frac{15.3/1.00g}{63.0/5.00g}\right) \\ =1.61×{10}^{3}y \end{gathered}$$

Hence, the charcoal is $1.61×{10}^{3}y$old.