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What is the osmotic pressure of a solution made by dissolving 60.0 g of glucose, C₆H₁₂O₆, in enough water to form 800.0 mL of solution at 45.0 °C ? Express your answer to three significant figures and include the appropriate units.

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Answer:

The osmotic pressure is 10.8 atm

Explanation:

Formula for osmotic pressure is:

π = M . R . T

where M is molarity (mol/L)

R, Universal gas constant (0.082 l.atm/mol.K)

T, T° in K (T°C + 273)

π = M . 0.082 l.atm/mol.K . 318K

Let's calculate the molarity

In 800 mL ____ 60 g

1000 mL _____ 75 g

This is the mass in 1L of solution.

Molar mass glucose = 180.15 g/m

Mass / Molar mass = 75 g/ 180.15 g/m → moles

Moles = 0.416M

π = 0.416 mol/l . 0.082 l.atm/mol.K . 318K

π = 10.8 atm

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