An aqueous solution at 27°c contains 3.6 g of a protein in a 200 ml sample. the osmotic pressure is 0.0203 atm. what is the mola

Question

Lady_Fox [76]

4 years ago

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An aqueous solution at 27°c contains 3.6 g of a protein in a 200 ml sample. the osmotic pressure is 0.0203 atm. what is the mola

r mass of the protein

Chemistry

1 answer:

umka21 [38] · Answer 1 · 2021-11-13T11:02:37+03:00

In order to calculate the molar mass of the protein, we may manipulate the ideal gas equation:
PV = nRT, where n is the number of moles. We also know that:
n = m / Mr, where m is mass and Mr is molecular weight
Thus,
Mr = (mRT)/(PV)
Here, the mass is in grams, the temperature is in Kelvin, the pressure is in atm and the volume is in liters, so the molar gas constant is 0.082057.

Mr = (3.6 * 0.082057 * (27 + 273)) / (0.0203 * 0.2)
Mr = 21,828 g/mol
Thus, the Mr of the protein is 2.18 x 10⁴ g/mol