Understanding the Experiment
In this experiment, we are evaluating the weight of oxygen (O₂) filled in a pre-weighed vessel at Normal Temperature and Pressure (N.T.P.) and then replacing it with sulfur dioxide (SO₂) after evacuation.
Key Concepts
- N.T.P. Conditions: Normal Temperature and Pressure is defined as 0°C (273.15 K) and 1 atm pressure. Under these conditions, the molar volumes of gases are standardized.
- Molar Masses:
- Oxygen (O₂) has a molar mass of approximately 32 g/mol.
- Sulfur Dioxide (SO₂) has a molar mass of approximately 64 g/mol.
Weight Determination
- When the vessel is filled with O₂ at N.T.P., the weight can be calculated using the ideal gas law. The number of moles of O₂ can be determined based on the molar volume (22.4 L/mol at N.T.P.).
- After the vessel is evacuated and filled with SO₂, the weight change can be determined by the difference in weight before and after filling.
Weight Calculation
- Let the volume of the vessel be V liters.
- The weight of oxygen can be calculated as:
- Weight of O₂ = (Molar mass of O₂) × (Number of moles of O₂)
- Number of moles of O₂ = Volume (V) / Molar volume (22.4 L)
- Therefore, Weight of O₂ = (32 g/mol) × (V / 22.4 L)
- After filling with SO₂, the weight would change similarly based on the molar mass of SO₂.
Conclusion
- By knowing the volume of the vessel and the molar mass of O₂, we can accurately determine the weight of oxygen initially filled in the vessel. This approach highlights the relationship between gas properties and molar mass at standardized conditions.