Mass of flask and foil(g) - 64.5297g Mass of flask, foil and condensed vapor - 6

Question

Mass of flask and foil(g) - 64.5297g Mass of flask, foil and condensed vapor - 64.9787g Temperature of boiling water bath - 101.2 C Volume of flask (mL) - 153.0 Barometric pressure - 762.4 mmHg Room temp - 23 C Vapor pressure at room temperature - 100 mmHg Calculate: 1. Uncorrected mass of condensed vapor(g) 2. Corrected density of air(g/L) 3. Average volume of flask (L) 4. Initial mass of air in flask (g) 5. Final partial pressure of air in flask (mmHg) 6.FInal mass of air in flask (g) 7.Mass of air lost (g) 8. Corrected mass of condensed vapor(g) 9. Molecuular weight (g/mol)

density Final partial pressure of onE air in flask Final mass of air in flask Mass of air lost Corrected mass of condensed vapor Molecular weight of unknown liquid 172 EXPERIMENT 10

Explanation / Answer

Solution:

1. Mass of condensed vapor = 64.9787 - 64.5297 g = 0.449 g

2. Mass of flask and foil + air = 64.5297g.

Mass of condensed vapor = 0.449 g

Therefore, mass of flask, foil + air = 64.5297 – 0.449 = 64.0807 g

Now by knowing mass of (flask + foil) we can calculate mass of air in the flask and its density.

3. Average volume of flask (L) = 0.153 L

4. Density of air at room temperature (23oC) = 1.27 kg/m3 = 1.27x10-3 g/mL

V1 = 153 mL.

We know: D = M/V1

or, M(air) = DV1 = 1.27x10-3x153 = 0.194 g

5. Given:

Temperature of boiling water bath (T2) = 101.2 oC = 374.2 K

Volume of flask (mL) = V1 = V2 = 153.0 mL

Barometric pressure = 762.4 mmHg.

Room temp (T1) = 23 oC = 296 K

Vapor pressure at room temperature (P1) = 100 mmHg.

We know that:

P1V1/T1 = P2V2/T2

Or, P2 = P1V1T2/V2T1

            = 100x153x374.2/153x296

            = 126.41 mmHg

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