Finding the Molar Mass Difference Between Carbon Dioxide and Air
Summary
The molar mass of an ideal gas is directly proportional to its density. This property has long been used in laboratory experiments in which a flask is filled with the vapor of a volatile liquid, and the mass, volume, temperature, and pressure of the vapor are used to find the molar mass of that vapor. In a related approach, the difference in the mass between a sample of carbon dioxide and a sample of air with the same volume, temperature, and pressure can be used to find the difference between the molar mass of the two gases. Using a balance, the mass of a flask filled with carbon dioxide gas sublimed from dry ice can be compared to the same flask filled with air to estimate the difference in molar mass between the gas systems.
Safety Precautions, Hazards, and Risk Assessment
Chemicals and their CAS numbers.
Dry ice (carbon dioxide) 124-38-9
Precautions, including proper personal protective equipment such as goggles and gloves, should be used when working with experiments. There is always a chance glass could break from thermal shock. Always wash your hands after completing the experiments and demonstrations.
Dry ice (carbon dioxide) 124-38-9
Precautions, including proper personal protective equipment such as goggles and gloves, should be used when working with experiments. There is always a chance glass could break from thermal shock. Always wash your hands after completing the experiments and demonstrations.
Teacher Recommendations or Piloting Data (if available)
Described in the attached file.
Digital Object Identifier (DOI)
https://doi.org/10.59877/RZFU7280
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