Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question

How would you solve the fifth question (there is only one trial to calculate the molar mass of butane for)?

Data Table: Analysis: 1. - 2. 3. 4. 5. 6. 7. 8. 9. 10. 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) nt lighter for each trial. ss of each of the butane lighters to the nearest 0.1 1 2 13.35099 13.24820 22.4°C 4482 mL 29.85 ing 20.45 3 AWOWO 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. Calculate the mass of butane collected for each trial. Calculate the molar mass of butane gas for each trial. 1 molar = mass mass Molar Mass= Mass / # of moles VT Calculate the average molar mass of butane. Determine the formula of butane and the accepted molar mass of butane. Calculate the n percent error in your experimentally determined molar mass. PV=nR If some bubbles of butane escape and are not collected in the eudiometer, how will the experimentally determined molar mass be affected? You would think the malar If an air bubble is left in the eudiometer before the collected, how will the experimentally determined molar mass be affected? 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?
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Transcribed Image Text:Data Table: Analysis: 1. - 2. 3. 4. 5. 6. 7. 8. 9. 10. 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) nt lighter for each trial. ss of each of the butane lighters to the nearest 0.1 1 2 13.35099 13.24820 22.4°C 4482 mL 29.85 ing 20.45 3 AWOWO 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. Calculate the mass of butane collected for each trial. Calculate the molar mass of butane gas for each trial. 1 molar = mass mass Molar Mass= Mass / # of moles VT Calculate the average molar mass of butane. Determine the formula of butane and the accepted molar mass of butane. Calculate the n percent error in your experimentally determined molar mass. PV=nR If some bubbles of butane escape and are not collected in the eudiometer, how will the experimentally determined molar mass be affected? You would think the malar If an air bubble is left in the eudiometer before the collected, how will the experimentally determined molar mass be affected? 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?
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