Answer:
A = 0.84
Step-by-step explanation:
The absorbance of the myoglobin solution can be calculated by using the Beer-Lambert law:
[tex] A = \epsilon*C*l [/tex]
Where:
A: is the absorbance
ε: is the molar attenuation coefficient = 15,000 M⁻¹cm⁻¹
l: is the optical path length = 1 cm
C: is the concentration = 1 mg/ml
Since the concentration is given in mg/ml and the molar attenuation coefficient is given in M (mol/L) we need to convert the concentration in mg/ml to mol/L and for that, we need to use the molecular weight of myoglobin = 17.8 kDa = 17.8x10³ g/mol:
[tex] C = 1 \frac{mg}{ml} \cdot \frac{1 g}{1000 mg} \cdot \frac{1000 ml}{1 L} \cdot \frac{1 mol}{17.8\cdot 10^{3} g} = 5.62 \cdot 10^{-5} mol/L [/tex]
Now, we can calculate the absorbance of the myoglobin:
[tex]A = 15,000 L*mol^{-1}*cm^{-1}*5.62\cdot 10^{-5} mol*L^{-1}*1 cm = 0.84[/tex]
Therefore, the absorbance of the myoglobin solution is 0.84.
I hope it helps you!
