The solvent for an organic reaction is prepared by mixing 50.0 of acetone () with 61.0...

The solvent for an organic reaction is prepared by mixing 50.0 of acetone () with 61.0 of ethyl acetate (). This mixture is stored at 25.0 . The vapor pressure and the densities for the two pure components at 25.0 are given in the following table. What is the vapor pressure of the stored mixture?

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Expert Solution

The units are not given. As these are liquids we assume the unit is mL.

Density of Acetone is 0.791 g/mL.

So, mass of 50.0 mL of Acetone is (50.0 * 0.791) g = 39.55 g.

Molar mass of Acetone is 58.08 g/mol.

Number of moles of Acetone is (39.55/58.08) mol = 0.68 mol.

Density of Ethyl acetate is 0.897 g/mL.

So, mass of 61.0 mL of Ethyl acetate is (61.0 * 0.897) g = 54.72 g.

Molar mass of Ethyl acetate is 88.11 g/mol.

Number of moles of Ethyl acetate is (54.72/88.11) mol = 0.62 mol.

Total number of moles is (0.68+0.62) mol = 1.30 mol.

Mole fraction of Acetone is (0.68/1.30) = 0.52

Mole fraction of Ethyl acetate is (0.62/1.30) = 0.48

The vapor pressure of a binary mixture with mole fractions X_A and X_B is expressed as

P = X_A * P⁰_A + X_B * P⁰_B

Using this formula and putting the vapour pressure of the pure components from the table the total pressure is calculated.

queen_honey_blossom answered 7 months ago

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