Mole Fraction.

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Presentation transcript:

Mole Fraction

Mole Fraction (X) is the number of moles of that component divided by the total number of moles of solute and solvent. X = Moles of component Total moles of solution

Mole Fraction (X) XSolute = Moles of solute Total moles of solution XSolvent = Moles of solvent Where: Xsolute + XSolvent = 1

1. An industrial gas contains 64. 0g of SO2 in every 750. 0g of CO2 1. An industrial gas contains 64.0g of SO2 in every 750.0g of CO2. What is the mole fraction of SO2? Given: Mass of Solute – 64.0 g Mass of Solvent – 750.0 g Formula: X = Moles of component Total moles of solution Answer: Moles solute = Mass of Solute Molar Mass of Solute = 64.0 g 32+ (16)2g/mole = 1 mole Answer: Moles solvent = Mass of Solvent Molar Mass of Solvent = 750.0 g 12+ (16)2g/mole = 17.05 mole

Given: Moles of Solute – 1 mole Moles of Solvent – 17 Given: Moles of Solute – 1 mole Moles of Solvent – 17.05 moles Formula: Mole Fraction = Moles of component Total moles of solution Answer: XSO2 = Moles of SO2 Total moles of Solution = 1 mole 1 + 17.05 mole = 0.05540

2. 100 mole of NaCl is dissolved into 100. 0 grams of pure H2O 2. 0.100 mole of NaCl is dissolved into 100.0 grams of pure H2O. What is the mole fraction of NaCl? Given: Mole of Solute – 0.100 mole Mass of Solvent – 100.0 g Formula: X = Moles of component Total moles of solution Answer: Moles solvent = Mass of Solvent Molar Mass of Solvent = 100.0 g 2 + 16 g/mole = 5.56 mole Answer: XNaCl = Moles of NaCl Total moles of Solution = 0.100 mole 5.56 + 0.100 mole = 0.018

SEATWORK 1. A 12.60 g isopropyl alcohol (C3H7OH) is dissolved in a 80 g of water. Calculate mole fraction of isopropyl alcohol in the solution.

Given: Mass of Solute – 12. 60 g Mass of Solvent – 80 Given: Mass of Solute – 12.60 g Mass of Solvent – 80.0 g Formula: X = Moles of component Total moles of solution Answer: Moles solute = Mass of Solute Molar Mass of Solute = 12.60 g (12)3 + (1)8 + 16 g/mole = 0.21 mole Answer: Moles solvent = Mass of Solvent Molar Mass of Solvent = 80.0 g 2 + 16 g/mole = 4.44 mole

Given: Moles of Solute – 0. 21 mole Moles of Solvent – 4 Given: Moles of Solute – 0.21 mole Moles of Solvent – 4.44 moles Formula: X = Moles of component Total moles of solution Answer: XSolute = Moles of C3H7OH Total moles of Solution = 0.21 mole 0.21 + 4.44 mole = 0.045