Use the References to access important values if needed for

Use the References to access important values if needed for this question In a laboratory experiment, a student found that a 186-mL, aqueous solution containing 2.329 g of a compound had an osmotic found to be nonvolatile and a nonelectrolyte. What is the molar mass of this compound? 2329 g of a compound had an osmotic pressure of 12.5 mm Hg at 298 K. The compound was also g mol Submin Answer

Solution

Answer:

From the ideal gas equation PV=nRT

Where P=pressure, V=volume, n=number of moles=mass/molar mass,

R=gas constant=0.0821 L atm/mol.K and T=temperature.

Given P=12.5 mmHg, since 1mmHg=0.00131atm then 12.5 mmHg=0.0164 atm.

V=186 ml=0.186 L, T=298 K and mass=2.329 g.

Molar mass=?

PV=(mass/molar mass)RT

Molar mass=(mass x RT)/PV

Molar mass=(2.329g x 0.0821Latm/mol.K x 298 K)/(0.0164 atmx0.186L)

Molar mass=18679.8 g/mol.