Question

A solution of 62.4 g of insulin in enough water to make 1.000 L of solution has an osmotic pressure of 0.305 atm at 25°C. Based on these data, what is the molar mass of insulin?

Answer 1

Molecular Mass of insulin = 5004

Step-by-step explanation:

Mass of insulin = 62.4 g

Volume of the solution = 1.00 L

Osmotic pressure = 0.305 L

Temperature = 25 °C = 25 + 273 = 298 K

PV = nRT

Where,

P = osmotic pressure

V = Volume of the solution

n = No. of moles

R gas constant = 0.08206 L atm K^{-1} Mol^{-1}

T = Temperature

PV = nRT

`n=(PV)/(RT)`

`n=((0.305 atm)(1.00 L))/((0.08206  L atm K^(-1) Mol^(-1))(298 K))`

n = 0.01247

No. of mol = Mass in g/molecular mass

Molecular mass = Mass in g/No. of mol

Molecular mass = 62.4/0.01247

= 5004