Answer:
The molar mass of the protein is 12982.8 g/mol.
Explanation:
The osmptic pressure is given by:
π=MRT
Where,
M: is molarity of the solution
R: the ideal gas constant (0.0821 L·atm/mol·K)
T: the temperature in kelvins
Hence, we look for molarity:
[tex]0.138 atm=M(0.0821\frac{l*atm}{mol*K} )(28+273K)[/tex]
[tex]M=\frac{0.138atm}{(0.0821\frac{l*atm}{mol*K} )(301K)}[/tex]= =5.584×10⁻³mol/l
As we have 2 ml of solution, we can get the moles quantity:
Moles of protein: 5.584×10⁻³[tex]\frac{mol}{l}\frac{1l}{1000ml}[/tex]×2ml=1.117×10⁻⁵mol
Finally, the moles quantity is the division between the mass of the protein and the molar mass of the protein, so:
Moles=Mass/Molar mass
Molar mass= Mass/Moles=[tex]\frac{0.145g}{1.117*10^{-5}mol}[/tex]=12982.8 g/mol
