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 =
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 =
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
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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)?
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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