Verification of the Molecular Formula and Percent Composition of the Compound, Magnesium Oxide
The Verification of the Molecular Formula and Percent Composition of the Compound Magnesium Oxide (MgO) Nice sounding title
Date Performed Lab: 8/31/06
Purpose: The purpose of this lab was to confirm the chemical formula of magnesium oxide by comparing 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. Using molar masses of both magnesium and oxygen, an expected percent composition, by mass, was found and compared to our experimental results.
Procedure: Find the mass of a clean crucible and cover. Add 8 inches of coiled magnesium ribbon to the crucible and mass again. Heat the crucible with cover slightly ajar and remove from heat when there is no more glow or shiny metallic pieces. Break up the remaining solid and add water. Heat the crucible to remove all water. Find the mass. good
Procedure:
Add magnesium in a clean crucible and heat the crucible with a small flame. Check the magnesium periodically and wait until the shiny appearances of the magnesium turn to grayish-white powdered oxide. Add water to the crucible and heat until the water is driven off; the expelled steam should make the pH paper bluish. Good and concise.
Calculations:
1. Initial weight of magnesium-
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2. Weight of magnesium oxide present after reaction-
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3. Percentage of magnesium in the magnesium oxide from experimental data-
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4. Theoretical percentage of magnesium (by mass) in magnesium oxide-
[pic][pic]
5. Percentage Error- [pic] Nice looking calculations
Conclusion
In conclusion, we were able to confirm that the formula for magnesium oxide is MgO. Using the masses of Mg and MgO that we calculated from our experiment, we determined that the percent composition of Mg in MgO is 57.5937%. The actual percent composition is 60.304%. We had 4.4947% error.
Conclusions:
Date Performed Lab: 8/31/06
Purpose: The purpose of this lab was to confirm the chemical formula of magnesium oxide by comparing 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. Using molar masses of both magnesium and oxygen, an expected percent composition, by mass, was found and compared to our experimental results.
Procedure: Find the mass of a clean crucible and cover. Add 8 inches of coiled magnesium ribbon to the crucible and mass again. Heat the crucible with cover slightly ajar and remove from heat when there is no more glow or shiny metallic pieces. Break up the remaining solid and add water. Heat the crucible to remove all water. Find the mass. good
Procedure:
Add magnesium in a clean crucible and heat the crucible with a small flame. Check the magnesium periodically and wait until the shiny appearances of the magnesium turn to grayish-white powdered oxide. Add water to the crucible and heat until the water is driven off; the expelled steam should make the pH paper bluish. Good and concise.
Calculations:
1. Initial weight of magnesium-
[pic]
2. Weight of magnesium oxide present after reaction-
[pic]
3. Percentage of magnesium in the magnesium oxide from experimental data-
[pic]
4. Theoretical percentage of magnesium (by mass) in magnesium oxide-
[pic][pic]
5. Percentage Error- [pic] Nice looking calculations
Conclusion
In conclusion, we were able to confirm that the formula for magnesium oxide is MgO. Using the masses of Mg and MgO that we calculated from our experiment, we determined that the percent composition of Mg in MgO is 57.5937%. The actual percent composition is 60.304%. We had 4.4947% error.
Conclusions: