Respuesta :
Answer:The molar mass of the protein is 16,544 g/mol.
Explanation:
Volume of the solution ,V = 2.00 ml= 0.002 L
Osmotic pressure [tex]\pi[/tex] = 0.138 atm
temperature at which solution is prepared = 28° C = 301 K([tex]0^oC=273 K[/tex])
Number of moles of protein,n=[tex]\frac{\text{Mass of the protein}}{\text{Molar mass of the protein}}=\frac{0.185 g}{M}[/tex]
Osmotic pressure is determined by :
[tex]\pi=\frac{n}{V}\times RT[/tex]
[tex]0.138 atm=\frac{0.185 g}{M\times 0.002 L}\times 0.0820 atm L/ mol K\times 301 K[/tex]
[tex]M=16,544 g/mol[/tex]
The molar mass of the protein is 16,544 g/mol.
The molar mass of the protein : 16517.86 g/mol
Further explanation
Osmosis pressure is the minimum pressure given to the solution so that there is no osmotic displacement from a more dilute solution to a more concentrated solution.
General formula:
[tex] \large {\boxed {\bold {\pi \: = \: M \: x \: R \: x \: T}}} [/tex]
π = osmosis pressure (atm)
M = solution concentration (mol / l)
R = constant = 0.08205 L atm mol-1 K-1
T = Temperature (Kelvin)
Mass of a protein: 0.185 g
Volume: 2.00 ml of solution. at 28 C
the osmotic pressure: 0.138 atm
We enter into the equation to find moles from protein concentrations
π = M. R. T
t = 28 C + 273 = 301 K
0.138 = M. 0.08205. 301 K
[tex]\rm M=\dfrac{0.138}{0.08205\times 301}\\\\M=0.00559[/tex]
[tex]\rm mol\:protein=volume\times molarity\\\\mol\:protein=0.002\times 0.00559\\\\mol=1.12.10^{-5}[/tex][/tex]
[tex]\rm molar\:mass=\dfrac{mass}{mol}\\\\molar\:mass=\dfrac{0.185}{1.12.10^{-5}}\\\\molar\:mass=16517.86[/tex]
Learn more
colligative properties
brainly.com/question/8567736
Raoult's law
brainly.com/question/10165688
The vapor pressure of benzene
brainly.com/question/11102916
The freezing point of a solution
brainly.com/question/8564755
brainly.com/question/4593922
brainly.com/question/1196173
