Data Table: Analysis: 1. 2. 3. mg. 4. 5 Use a different lighter for each trial. find and record the mass of each of the butane lighters to the nearest 0.1 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 4482mL 29.85 int 20.45 2 3 W 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 = mas mass V₁
Data Table: Analysis: 1. 2. 3. mg. 4. 5 Use a different lighter for each trial. find and record the mass of each of the butane lighters to the nearest 0.1 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 4482mL 29.85 int 20.45 2 3 W 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 = mas mass V₁
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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How would you solve the fourth question?
Transcribed Image Text:13.
Data Table:
Analysis:
1.
2.
3.
4.
5.
6.
7.
8.
9.
process for a second and third trial. Use a different lighter for each trial.
The next day, find and record the mass of each of the butane lighters to the nearest 0.1
mg.
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)
1
2
Proqui
13.35099
13.24820
22.4°C
44.82 mL
29.85 ing
20.45
ens va
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.
Calculate the mass of butane collected for each trial.
Calculate the molar mass of butane gas for each trial.
Molar Mass = Mass / # of moles
n=
Calculate the average molar mass of butane.
Determine the formula of butane and the accepted molar mass of butane. Calculate the
PV=nRT
percent error in your experimentally determined molar mass.
If some bubbles of butane escape and are not collected in the eudiometer, how will the
You would think the maar
experimentally determined molar mass be affected? You Would think the malar
mass
If an air bubble is left in the eudiometer before the gas is 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,
ally determined molar mass be affected?
1 mol = mass
mass
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