Constants I Periodic Table Consider two solutions, one formed by adding 10 g of

Question

Constants I Periodic Table Consider two solutions, one formed by adding 10 g of glucose (C6 H 206) to 1 L of water and the other formed by adding 10 g of sucrose (C12H22O1n) to 1 L of water Part A Calculate the vapor pressure for the first solution at 20 °C. (The vapor pressure of pure water at this temperature is 17.5 torr.) Express your answer using three significant figures torr Submit Request Answer Part B Calculate the vapor pressure for the second solution at 20 °C. (The vapor pressure of pure water at this temperature is 17.5 torr.) Express your answer using three significant figures torr Submit Request Answer

Explanation / Answer

Part A

Answer

17.48torr

Explanation

According to Raoult's law

Psolution = Xsolvent × P°solvent

where,

Psolution = Vapor pressure of solution

Xsolvent = mole fraction of solvent

P°solvent = Vapor pressure of solvent in its pure form

no of moles of C6H12O6 = 10g/180.156g/mol = 0.05551

no of moles of water = 1000g/18.02g/mol = 55.49

Total moles = 0.05551 + 55.494 = 55.55

mole fraction of water = 55.494/55.55 = 0.9990

Psolution = 0.9990× 17.5torr = 17.48torr

Part B

Answer

Psolution = 17.49

Explanation

No of moles of Sucrose =10g /342.297g/mol = 0.02921

No of moles of water = 55.494

Total no of moles = 55.494 + 0.02921 = 55.523

mole fraction of water = 55.494/55.523 = 0.9995

Psolution = 0.9995×17.5torr = 17.49

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