15 sis: 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 ML 29.85 ing 20.45 2 Calculate the mass of butane collected for each trial. Calculate the molar mass of butane gas for each trial. Mola 3 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. molar ma mast =

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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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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?
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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