A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as NV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.) %3D

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A certain dilute solution has an osmotic pressure of
11.1 atm at 25°C. Calculate the difference between
the chemical potential of the solvent in the solution
and that of pure water. Assume that the density is
the same as that of water at 25°C, 0.99705 g-cm-3.
(Hint: Express the chemical potential in terms of
mole fraction, x1, and rewrite the osmotic pressure
equation as OV = n2RT, where n2 is the number of
moles of the solute and V = 1.00 L.)
Transcribed Image Text:A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)
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