Answer:
The value of molar absorptivity of the compound is [tex]800 L mol^{-1} cm^{-1}[/tex].
Explanation:
Using Beer-Lambert's law :
[tex]A=\epsilon \times C\times l[/tex]
A = absorbance of solution
C = concentration of solution = [tex]2.00\times 10^{-3}M[/tex]
l = path length = 1.00 cm
[tex]\epsilon[/tex] = molar absorptivity coefficient
[tex]Concentration (C)= \frac{\text{moles of compound}}{\text{Volume of the solution(L)}}[/tex]
Moles of compound = [tex]\frac{1 mg}{160 g/mol}=\frac{0.001 g}{160 g/mol}=6.25\times 10^{-6} mol[/tex]
Volume of the solution = 10 mL = 0.010 L
[tex]C=\frac{6.25\times 10^{-6} mol}{0.010 L}=0.000625 mol/L[/tex]
A = 0.50 , l = 1 cm
[tex]0.50=\epsilon \times 0.000625 mol/L\times 1 cm[/tex]
[tex]\epsilon =\frac{0.50}{0.000625 mol/L\times 1 cm}=800 L mol^{-1} cm^{-1}[/tex]
The value of molar absorptivity of the compound is [tex]800 L mol^{-1} cm^{-1}[/tex].
