Respuesta :
Answer:
[tex]51.74 M^{-1} cm^{-1}[/tex] is the molar absorptivity constant for the dye.
Explanation:
Using Beer-Lambert's law :
[tex]A=\epsilon \times C\times l[/tex]
where,
A = absorbance of solution
C = concentration of solution =
[tex]\epsilon [/tex] = Molar absorptivity constant
l = path length
Given : C = 0.0003 M , l = 1 cm
[tex]\epsilon = ?[/tex]
[tex]\ln A_o=-4.1655[/tex]
[tex]A=e^{-4.1655}=0.01552[/tex]
[tex]0.01552=\epsilon \times 0.0003 M\times 1 cm[/tex]
[tex]\epsilon =\frac{0.01552}{0.0003 M\times 1 cm}=51.74 M^{-1} cm^{-1}[/tex]
[tex]51.74 M^{-1} cm^{-1}[/tex] is the molar absorptivity constant for the dye.
The molar absorptivity constant is a measure of the probability of an electronic transition. Assuming the path length is 1 cm, the molar absorptivity constant for the dye is 51.74 M.
What is the molar absorptivity constant?
Molar absorptivity ∈, also known as molar extinction coefficient, is a measure of the probability of an electronic transition.
Given,
By Beer's Lambert law
[tex]\bold{\epsilon\times C \times l }[/tex]
Concentration of the dye is 0.0003 M
ln (A0) = -4.1655
[tex]\bold{ A = e^-^4^.^1^6^5^5= 0.01552 }\\\\\bold{ 0.01552 = \epsilon \times 0.0003\;M\times 1\;cm }\\\\\\\bold{\epsilon=\dfrac{0.01552}{0.0003\;M\times 1\;cm} = 51.74\;M^-^1\;cm^-^1 }[/tex]
Thus, the molar absorptivity constant for the dye is 51.74 M.
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