CHEM 110 Exp08 Data Sheet
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docx
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Uploaded by gabriellehouseholder13
Community College of Philadelphia
Department of Chemistry
Lab Report Experiment 8 – Molar Mass of Magnesium
Name: Gabrielle Householder
Submitted Date: 04/03/2024
Lab Partners Thays
Laboratory Instructor: Michael Gregor
Lecture Instructor: Edogri
Experiment Nbr.: 8
Experiment Title: Ideal gas law Estimation of molar mass of magnesium
Purpose: to perform a oxidation- reeducation reaction, redox, involving the evolution of a gas. oxidation-reduction refers to chemical reactions in which there is a transfer of electrons. the loss of electrons is known as oxidation and the gain of electrons is reduction.
To use stoichiometry it is the study of the mole relationship between elements and compounds in chemical reaction To use ideal gas law PV=nRT
Error Analysis & Conclusion: My Findings reveals discrepancies between the experimental molar mass of magnesium (18.72g/mol) and the accepted value (24.67g/mol). Potential sources of error include inaccuracies in measurement devices, assumptions of ideal gas behavior, procedural errors, and uncertainties in handling equipment. Despite these discrepancies, the analysis provides valuable insights for refining experimental techniques and enhancing accuracy in future investigations. Further validation and exploration of factors influencing gas behavior are recommended to improve the reliability of molar mass determinations.
Data Sheet & Results: [] Attached
[Comments]
Lab Pre/Post Questions:
[] Attached
[Comments]
CHEM
110 EXP
08 DATA
SHEET
1
of 3
Community College of Philadelphia
Department of Chemistry
Lab Report Experiment 8 – Molar Mass of Magnesium
Ideal Gas Law = PV=nRT P-pressure, V-volume, n-moles, T-temperature (Kelvin)
R=ideal gas constant (0.0821 (L)(atm)/(mole)(Kelvin))
Reaction: Mg(s) = 2H
+
(aq) + H
2
(g)
#
Trial 1
Trial 2
Trial 3
1
Mass of Magnesium
0.053
2
Volume of Hydrogen Gas (mL)
71.2mL
3
Volume of Hydrogen Gas (L)
0.0712 L
4
Temperature of Gas (Celsius)
25 C
5
Temperature of Gas (Kelvin)
298 K
6
Atmospheric Pressure (mmHg)
762 mmHg
7
Vapor pressure of Water (mmHg)
(According to chart)
23.8 mmHg
8
Height of Water Column (mm)
(Difference in water levels)
209 mm
9
Mercury Equivalent Height
(line 8/13.6) = P
col
(mmHg)
15.37 mmHg
10
Pressure of Hydrogen (mmHg)
722.8 mmHg
11
Pressure of Hydrogen (atm)
0.951 atm
12
Moles of Magnesium
0.00277 mol
13
Calculated Molar Mass of Magnesium (g/mol Mg)
18.72g/mol
14
Avg Molar Mass
24.67 g/mol
15
% Error
-21.23%
SHOW % ERROR Calculation: Percentage Error= ∣Accepted Value|
|Experimental Value−Accepted Value
∣ ×100%
CHEM
110 EXP
08 DATA
SHEET
2
of 3
Community College of Philadelphia
Department of Chemistry
Lab Report Experiment 8 – Molar Mass of Magnesium
Consult the laboratory manual for additional information.
PRE & POST LAB Questions
Complete the pre and post lab questions with the provided MS Excel file. Copy your calculation into the Word document or submit the Excel file (rename file).
1
.
A 0.0500-g sample of magnesium is reacted with 25 mL 3.0 M sulfuric acid as described in the experimental section. The resulting hydrogen gas is collected over water and is found to have a volume of
51.0 mL The temperature is 25˚C and the atmospheric pressure is 760.00 mmHg. The column of water height inside the graduate cylinder is found to be 24.0 mm. 24.04 g/mol
2.
A 0.0524-g sample of magnesium is reacted with 25 mL 3.0 M sulfuric acid as described in the experimental section. The resulting hydrogen gas is collected over water and is found to have a volume of
53.6 mL The temperature is 25˚C and the atmospheric pressure is 762.12 mmHg. The column of water height inside the graduate cylinder is found to be 22.9 mm.
23.71g/mol
CHEM
110 EXP
08 DATA
SHEET
3
of 3
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