Dumas Method lab report (1)
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Name: Fauzia Ali Hassan Student Number: 069-068-519
Date Conducted: Feb 13rd, 2024
Date Submitted: Feb 26th, 2024
Partner’s Name: Rokaya Gamel
Lab Section: L6
Dumas Method for Determining The Molecular Weight of Volatile Liquids.
Abstract: This experiment had the objective to identify a material that was unknown by applying the ideal gas law and the Dumas technique to determine its molecular weight. Using the ideal gas law, the mass, temperature, and volume were determined to get the molecular weights. Weighing was done using a rubber band around a 50 ml Erlenmeyer flask and aluminium foil on top. 2 mL of acetone were then added. After the substance evaporated, the flask was submerged in a heated bath. It was determined what temperature the bath was. The flask was allowed to cool after the chemical vaporised before being weighed. This was done for at least three times to get trial 3 or 2. The weight of the material was determined by the difference between the weights before and after. The weight difference between an empty and full flask was used to compute the capacity. With this knowledge, the molecular weight of the unknown and acetone were determined using the ideal gas law. Ethanol was found to be the mystery solution, when the experiment was completed. This implies that a volatile liquid may be identified by its molecular weight using the Dumas method and the ideal gas law.
Procedure
For the procedure, see lab manual (CH110 Lab Manual, Winter 2024) pages 69-70. Wilfrid Laurier University Chemistry Department, Winter 2024, “Dumas Method for Determining The Molecular Weight of Volatile Liquids.” Pages 68- 73 in Chemistry 110 Lab Manual
.
Wilfrid Laurier University, ON, Canada.
Deviations occurred in this experiment: we used our own procedure to determine the flask volume and
one more trial was conducted in the experiment.
Table 1. Observations for determination of the molecular weight of acetone. Original mass of flask (g)
Mass of the flask after heating (g)
Mass of Acetone
Temperature (°)
Flask Used
Trial 1
39.6669g
39.7107
0.0438g
98.4°
1
Trial 2
39.6709
39.7083
0.0374 g
98.3°
1
Trial 3
38.6678
39.6749
1.0071
98.8°
1
Table 3. Observation for determination of molecular weight of unknown Original mass of flask (g) Mass of flask after heating (g)
Mass of unknown (g)
Temperature (°)
Flask Used Trial 1
40.3251g
40.3747 g
0.0496 g 98.4 °
2
Trial 2
40.3355g
40.4435 g 0.108 g
97.9°
2
Table 4. Qualitative Observation of Acetone In The Three Trials
Before During After Trial 1
Acetone : Unknown -
Clear, colourless liquid
Food Colouring -
Green, opaque
liquid Water Bath
-
Clear, transparent liquid Boiling chip
-
Small pieces of black porous rock solid.
Acetone + food colouring
-
Bubbles formed, food colouring dissolving, liquid was evaporated Unknown + food -
Bubbles formed, food colouring dissolving, liquid was evaporated
Acetone: -
Clear, Colourless gas
formed
Unknown: -
Clear, Colourless gas
formed
Trial 2
Acetone: Unknown -
Clear, colourless liquid
Food Colouring -
Green, opaque
liquid Water Bath
-
Clear, transparent liquid Boiling chip
-
Small pieces of black porous rock solid.
Acetone + food colouring
-
Bubbles formed, food colouring dissolving, liquid was evaporated Unknown + food -
Bubbles formed, food colouring dissolving, liquid was evaporated Acetone: -
Clear, Colourless gas
formed
Unknown: -
Clear, Colourless gas
formed
Trial 3
Acetone: Unknown
-
Clear, colourless liquid
Food Colouring -
Green, opaque
liquid Water Bath
-
Clear, transparent liquid Boiling chip
-
Small pieces of black porous rock solid. Acetone + food colouring
-
Bubbles formed, food colouring dissolving, liquid was evaporated Unknown + food -
Bubbles formed, food colouring dissolving, liquid was evaporated
Acetone: -
Clear, Colourless gas
formed
Unknown: -
Clear, Colourless gas
formed
Table 5. Data For Determination Of The Volume Of Flask Used. Temperature (°)
Mass of water in flask (g)
Density of water (g/ml) Volume of Flask
(mL) Flask 1
22.7°
56.0g 0.997612 g/mL
56.13 mL
Flask 2
23.9°
55.54
0.997446 g/mL
55.68 mL
Question. 1. Calculate the molecular weight of acetone and the unknown volatile liquid using the data obtained in your experiment for each trial. Then, calculate and report the average molecular weight of acetone and the unknown.
Sample Calculation 1: Calculation the molecular weight of acetone from trial 1. MW=mRT/PV
MW=[(0.0438g)(0.08206 L atm mol
−
¿
1 K −
1
) (371.55 K) / (1 atm) ( 0.05613L) ]
MW= 23.8 g/mol
Sample Calculation 2: Calculation the molecular weight of acetone from trial 2
MW=mRT/PV
MW= [(0.0374g)(0.08206 L atm mol
−
¿
1 K −
1
)(371.45 K)/ (1 atm) ( 0.05613L) ]
MW= 20.3 g/mol
Sample Calculation 3: Calculation the molecular weight of acetone from trial 3
MW=mRT/PV
MW= [(1.0071g)(0.08206 L atm mol
−
¿
1 K −
1
)(371.95 K)/ (1 atm) ( 0.05613L) ]
MW= 1.73g/mol Sample Calculation 4: Calculation the average molecular weight of acetone from all trials.
(23.8g/mol + 20.3 g/mol +1.73 g/mol) / 3 = 15.3g/mol
Sample Calculation 5: Calculation the molecular weight of unknown from trial 1
MW=mRT/PV
MW= [(0.0496g)(0.08206 L atm mol
−
¿
1 K −
1
)(371.55 K)/ (1 atm) ( 0.05568L) ]
MW= 27.2 g/mol
Sample Calculation 6: Calculation the molecular weight of unknown from trial 2
MW= [(0.108 g )(0.08206 L atm mol
−
¿
1 K −
1
)(371.05 K)/ (1 atm) (0.05568L) ]
MW= 59.1 g/mol
Sample Calculation 6: Calculation the average molecular weight of Unknown from all trials.
(27.16 g/mol + 59.06 g/mol ) / 2 = 43.1g/mol 2. From the molecular weight calculated in question 1, what is the unknown volatile liquid? Make your selection from the following list below. Include your unknown number somewhere in
your answer. -
The unknown has an average molecular weight of 43.1 g/mol, which is closer to ethanol's molecular weight of 46.06 g/mol.
3. Calculate the percent error for both acetone and the unknown volatile liquid. Sample Calculation 7: calculate the percent error for acetone. % Error = (Observed Value – Accepted Value)/(Accepted Value) x 100%
% Error= ( 15.27g/mol - 58.08 g/mol) / (58.08 g/mol) x
100%
% Error= -73.7% > = 73.7% Sample Calculation 7: calculate the percent error for unknown. % Error = (Observed Value – Accepted Value)/(Accepted Value) x 100%
% Error = ( 43.11 g/mol - 46.06 g/mol ) / (46.06 g/mol ) x 100%
% Error = -6.40% > = 6.40%
4. An alternative method of calculation for this experiment would be to calculate the volume of the gas at standard conditions and then use the molar volume at standard conditions to
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Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning