Determining the Empirical Formula of Magnesium Oxide
Chemistry
Practical Report:
Topic: Determining the Empirical Formula of Magnesium Oxide
Patrick Doan
11 CHEM 11
26/9/08
Table of contents
1.0 Aim 1
2.0 Theory 2-3
3.0 Materials 4
4.0 Method 4
5.0 Results 4 - 5.1 Qualitative Observations 4 - 5.2 Example Calculations for each Calculated Value 5-7 -5.21 Experimental Values and Associated Errors 5-7 - 5.3 Accumulated Raw Data 8 - 5.4 Mean Experimental Values and Associated Errors 8 - 5.5 Accumulated Calculated Values, Mean Values and Calculated Errors 9
6.0 Conclusion 10
7.0 Discussion 11 - 7.1 Comparison of Errors 11 - 7.2 Experimental Sources of Error 11
8.0 Bibliography 12
1.0 Aim:
The purpose of this experiment was to determine the empirical formula of magnesium oxide.
2.0 Theory:
The empirical formula also known as the chemical formula is the simplest molar combining ratio of elements in a compound. Thus, if to understand the behaviour of a chemical compound we must know its chemical formula. The molecular formula is the same as or a multiple of the empirical formula, and the actual number of atoms of each type in the compound. The ratio can be determined if the mass of the individual elements, in this case magnesium and oxygen, is known in a known mass of the compound. For example:
[pic][pic]
To verify the empirical formula of magnesium oxide was to compare the masses of pure magnesium solid prior to any reaction and magnesium oxide solid after a reaction between all of the magnesium and oxygen from the air when heated from a Bunsen burner in a crucible. The concept of the mole will lead to determining the empirical formula of magnesium oxide.
In this experiment, after a known mass of magnesium is combusted, the product will consist of magnesium oxide and smaller amounts of magnesium nitride. Water will convert the nitride to
Practical Report:
Topic: Determining the Empirical Formula of Magnesium Oxide
Patrick Doan
11 CHEM 11
26/9/08
Table of contents
1.0 Aim 1
2.0 Theory 2-3
3.0 Materials 4
4.0 Method 4
5.0 Results 4 - 5.1 Qualitative Observations 4 - 5.2 Example Calculations for each Calculated Value 5-7 -5.21 Experimental Values and Associated Errors 5-7 - 5.3 Accumulated Raw Data 8 - 5.4 Mean Experimental Values and Associated Errors 8 - 5.5 Accumulated Calculated Values, Mean Values and Calculated Errors 9
6.0 Conclusion 10
7.0 Discussion 11 - 7.1 Comparison of Errors 11 - 7.2 Experimental Sources of Error 11
8.0 Bibliography 12
1.0 Aim:
The purpose of this experiment was to determine the empirical formula of magnesium oxide.
2.0 Theory:
The empirical formula also known as the chemical formula is the simplest molar combining ratio of elements in a compound. Thus, if to understand the behaviour of a chemical compound we must know its chemical formula. The molecular formula is the same as or a multiple of the empirical formula, and the actual number of atoms of each type in the compound. The ratio can be determined if the mass of the individual elements, in this case magnesium and oxygen, is known in a known mass of the compound. For example:
[pic][pic]
To verify the empirical formula of magnesium oxide was to compare the masses of pure magnesium solid prior to any reaction and magnesium oxide solid after a reaction between all of the magnesium and oxygen from the air when heated from a Bunsen burner in a crucible. The concept of the mole will lead to determining the empirical formula of magnesium oxide.
In this experiment, after a known mass of magnesium is combusted, the product will consist of magnesium oxide and smaller amounts of magnesium nitride. Water will convert the nitride to
Bibliography: Elvins, Carolyn and others 2004, Heinemann Chemistry one 3rd Edition, Reed International Books Australia Pty Ltd, Port Melbourne, Victoria Microsoft Encarta Encyclopedia Standard, 2005, CD ROM, Microsoft Corporation, U.S.A Viewed 17th September Viewed 17th September Patrick Doan 12 ----------------------- [pic] [pic] [pic] [pic]