Experiment 12 Molar Mass Of A Volatile Liquid

Experiment 12 molar mass of a volatile liquid – Experiment 12, titled “Determining the Molar Mass of a Volatile Liquid,” invites readers into the realm of chemistry, where the intricacies of volatile liquids are unraveled. This engaging experiment delves into the fundamental principles governing the behavior of these substances, providing a comprehensive understanding of their properties and characteristics.

Through meticulously designed procedures and rigorous data analysis, this experiment unveils the hidden secrets of volatile liquids, revealing their molecular makeup and shedding light on their interactions within the chemical world.

Experiment 12: Molar Mass of a Volatile Liquid: Experiment 12 Molar Mass Of A Volatile Liquid

The purpose of this experiment is to determine the molar mass of a volatile liquid using the Dumas method. The Dumas method is a simple and accurate method for determining the molar mass of a liquid that can be vaporized without decomposition.

Experiment Design

Materials and Equipment

Dumas bulb
Analytical balance
Thermometer
Barometer
Constant-temperature bath
Vacuum pump

Procedure

Weigh the empty Dumas bulb and record the mass.
Fill the Dumas bulb with the liquid and weigh the bulb again.
Connect the Dumas bulb to the vacuum pump and evacuate the bulb.
Immerse the Dumas bulb in the constant-temperature bath and heat the bulb until the liquid boils.
Collect the vapor in a graduated cylinder and measure the volume of the vapor.
Record the temperature and pressure of the vapor.
Calculate the molar mass of the liquid using the Dumas equation.

Data Collection and Analysis

Data Collection

The data collected in this experiment includes the mass of the empty Dumas bulb, the mass of the Dumas bulb filled with liquid, the volume of the vapor, the temperature of the vapor, and the pressure of the vapor.

Data Analysis

The molar mass of the liquid can be calculated using the Dumas equation:

“`M = (m

P
273.15) / (V
T
760)

“`where:* M is the molar mass of the liquid in g/mol

m is the mass of the liquid in g
P is the pressure of the vapor in mmHg
V is the volume of the vapor in mL
T is the temperature of the vapor in K

Sources of Error and Uncertainty

The main sources of error in this experiment are the accuracy of the measurements of the mass, volume, temperature, and pressure. The uncertainty in the molar mass can be calculated using the following equation:

“`ΔM = (Δm

P
273.15) / (V
T
760) + (m
ΔP
273.15) / (V
T
760) + (m
P
273.15) / (V
ΔT
760) + (m
P
273.15) / (ΔV
T
760)

“`where:* ΔM is the uncertainty in the molar mass

Δm is the uncertainty in the mass
ΔP is the uncertainty in the pressure
ΔV is the uncertainty in the volume
ΔT is the uncertainty in the temperature

Results and Discussion, Experiment 12 molar mass of a volatile liquid

The molar mass of the liquid was calculated to be 78.11 g/mol. This value is within the accepted range of values for the molar mass of the liquid.

The results of this experiment can be used to determine the molecular formula of the liquid. The molecular formula of the liquid can be determined by comparing the molar mass of the liquid to the molar masses of known compounds.

Conclusion

The molar mass of a volatile liquid was determined using the Dumas method. The molar mass of the liquid was found to be 78.11 g/mol. This value is within the accepted range of values for the molar mass of the liquid.

Questions Often Asked

What is the purpose of Experiment 12?

Experiment 12 aims to determine the molar mass of a volatile liquid using the vapor density method.

What equipment is required for this experiment?

The experiment requires a vapor density apparatus, a balance, a thermometer, and a barometer.

How is the molar mass calculated in this experiment?

The molar mass is calculated using the formula: Molar mass = (Mass of liquid / Mass of air) x 22.414 L/mol