M6L1 Determination of Ideal Gas Law Constant 2022
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Determination of Ideal Gas Law Constant
April 6, 2021
Purpose
To understand the relationship between pressure and the number of moles of gas in order to determine the ideal gas law constant. Procedure
Comprise an apparatus to calculate the gas particles when
hydrogen peroxide and yeast are mixed. Experimental Data
Table 1
Include correct units with each data
Trial
1
Trial
2
Trial
3
Trial
4
Trial
5
Trial
6
Trial
7
Trial
8
Air temperature
22.2
C
22.2
C
22.2
C
22.2
C
22.2
C
22.2
C
22.2
C
22.2
C
Volume H
2
O
2
1ml
1ml
2ml
2ml
3ml
3ml
4ml
4ml
1
Trial
1
Trial
2
Trial
3
Trial
4
Trial
5
Trial
6
Trial
7
Trial
8
liquid Initial Volume
Gas
2ml
5ml
6ml
7ml
7ml
6ml
4ml
7ml
Final Volume Gas 9ml
11ml
20ml
19ml
50ml
30ml
40ml
40ml
ΔV 7ml
6ml
14ml
12ml
43ml
24ml
36ml
34ml
Table 2
Show reaction used to produce O
2 Include correct units with each data
Concentration H
2
O
2
Trial
1
Trial
2
Trial
3
Trial
4
Trial
5
Trial
6
Trial
7
Trial
8
Moles
H
2
O
2 2mol
2mol
4mol
4mol
6mol
6mol
8mol
8mol
Moles O
2 1mol
1mol
2mol
2mol
3mol
3mol
4mol
4mol
ΔV (L)
0.007
L
0.006
L
0.015
L
0.012
L
0.025
L
0.025
L
0.035
L
0.033
L
Show calculations:
© 2016 Carolina Biological Supply Company
2
Concentration of H
2
O
2
3g/34.01g/mol/0.1=0.882mol
Moles H
2
O
2
.882x.001=0.000882mol
Moles O
2
Insert graph of moles of O
2
vs. volume of O
2
. Label graph correctly. Add linear trendline.
Table 3
Include correct units with each data
Result Calculations
Air Temperature 295.2K
Air Pressure 1.0atm Equation of Line
from the graph
Y=18.25x
Gas Constant R
.882x.001=0.000882
mol M=RT/P Percent Error
24.8% 0.08206-
0.0617/0.08206X100=24.8%
© 2016 Carolina Biological Supply Company
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3
Lab Questions 1.
Would the volume of oxygen generated in the reaction change if a smaller
mass of yeast were used? Why or why not?
The volume of oxygen generated would not change if a smaller mass of yeast were used. This is because the yeast is a catalyst and a catalyst does not affect the reaction or the product.
2.
Which assumptions did you make in this experiment?
That the more product there was, the more gas particles there would be
3.
Identify at least two potential sources of experimental error.
User error when measuring the yeast and or hydrogen peroxide. Another
would be measuring the gas incorrectly.
Experimental Conclusions
This experiment helped me understand the relationship between pressure and the number of moles of gas to determine the ideal gas law constant Personal Reflection This was a cool lab. A bit messy due to the water but overall it was a cool lab
© 2016 Carolina Biological Supply Company
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MODEL: GASES EXERT PRESSURE INDEPENDENTLY
Condition Pressure
initial
final
1.0 atm
3.0 atm
Volume
22.4 L
22.4 L
Temperature
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Comment
1.0 mole of N₂ gas fills the tank.
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B. Direction: Complete the following table and use the Ideal gas equation to calculate
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Temperature (T)
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0.50 mol
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