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Analysis: 1. 2. 3. Trial number lighter number initial mass of lighter final mass of lighter (we'll get this after they have dried overnight) Temperature (read from thermometer) volume of butane (read from eudiometer tube) Barometric pressure (read from barometer) vapor pressure of water (read from chart of vapor pressures) 1 13.35099 13.24820 22.4°C 4482 MAL 29.85mg 20.45 2 3 MO Convert the barometric pressure from inHg to mmHg. (1 in = 25.4 mm) Use Dalton's Law to calculate pressure of the butane alone. Using the Ideal Gas Law, calculate the moles of butane for each trial using the ideal gas law.

Analysis: 1. 2. 3. Trial number lighter number initial mass of lighter final mass of lighter (we'll get this after they have dried overnight) Temperature (read from thermometer) volume of butane (read from eudiometer tube) Barometric pressure (read from barometer) vapor pressure of water (read from chart of vapor pressures) 1 13.35099 13.24820 22.4°C 4482 MAL 29.85mg 20.45 2 3 MO Convert the barometric pressure from inHg to mmHg. (1 in = 25.4 mm) Use Dalton's Law to calculate pressure of the butane alone. Using the Ideal Gas Law, calculate the moles of butane for each trial using the ideal gas law.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Educational Website Transcription:** ## Data Table: 1. **Trial Number**: 1 - **Lighter Number**: 1 - **Initial Mass of Lighter**: 13.3509 g - **Final Mass of Lighter**: 13.2482 g - **Temperature**: 22.4 °C (read from thermometer) - **Volume of Butane**: 148.2 mL (read from eudiometer tube) - **Barometric Pressure**: 29.85 inHg (read from barometer) - **Vapor Pressure of Water**: 20.4 mmHg (read from chart of vapor pressures) ## Analysis: 1. Convert the barometric pressure from inches of Hg to mmHg. (1 inch = 25.4 mm) 2. Use Dalton's Law to calculate the pressure of the butane alone. 3. Using the Ideal Gas Law, calculate the moles of butane for each trial. 4. Calculate the mass of butane collected for each trial. 5. Calculate the molar mass of butane gas for each trial. - **Formula**: Molar Mass = Mass / Number of Moles 6. Calculate the average molar mass of butane from all trials. 7. Determine the formula of butane and the accepted molar mass of butane. Calculate the percent error in your experimentally determined molar mass. 8. If some bubbles of butane escape undetected in the eudiometer, how will the experimentally determined molar mass be affected? 9. If an air bubble is left in the eudiometer before the gas is collected, how will the experimentally determined molar mass be affected? 10. If a student forgets to adjust the total pressure to calculate the pressure of just the butane, how will the experimentally determined molar mass be affected? **Note**: The table and analysis steps guide students on how to experimentally determine the properties of butane using the Ideal Gas Law and other related calculations. Calculations of pressures, molar mass determination, and error analysis are emphasized for educational purposes.
Transcribed Image Text:**Educational Website Transcription:** ## Data Table: 1. **Trial Number**: 1 - **Lighter Number**: 1 - **Initial Mass of Lighter**: 13.3509 g - **Final Mass of Lighter**: 13.2482 g - **Temperature**: 22.4 °C (read from thermometer) - **Volume of Butane**: 148.2 mL (read from eudiometer tube) - **Barometric Pressure**: 29.85 inHg (read from barometer) - **Vapor Pressure of Water**: 20.4 mmHg (read from chart of vapor pressures) ## Analysis: 1. Convert the barometric pressure from inches of Hg to mmHg. (1 inch = 25.4 mm) 2. Use Dalton's Law to calculate the pressure of the butane alone. 3. Using the Ideal Gas Law, calculate the moles of butane for each trial. 4. Calculate the mass of butane collected for each trial. 5. Calculate the molar mass of butane gas for each trial. - **Formula**: Molar Mass = Mass / Number of Moles 6. Calculate the average molar mass of butane from all trials. 7. Determine the formula of butane and the accepted molar mass of butane. Calculate the percent error in your experimentally determined molar mass. 8. If some bubbles of butane escape undetected in the eudiometer, how will the experimentally determined molar mass be affected? 9. If an air bubble is left in the eudiometer before the gas is collected, how will the experimentally determined molar mass be affected? 10. If a student forgets to adjust the total pressure to calculate the pressure of just the butane, how will the experimentally determined molar mass be affected? **Note**: The table and analysis steps guide students on how to experimentally determine the properties of butane using the Ideal Gas Law and other related calculations. Calculations of pressures, molar mass determination, and error analysis are emphasized for educational purposes.
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