Determination of the Formula of a metal oxide.docx - Purpose The purpose of this experiment is to prepare a metal oxide and determine its empirical

Determination of the Formula of a metal oxide.docx -...

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Purpose The purpose of this experiment is to prepare a metal oxide and determine its empirical formula. The experiment will also demonstrate the law of constant composition. Procedure The procedure for this lab can be found on pages 35- 39 in “General Chemistry CHEL-110 Laboratory Manual Fall 2017”. Data Tables Carbon copies have been attached to the back of this lab report. Calculations 1. Percent of Magnesium 0.157/ 24.31 X 100 = 55.67% 2. Percent of Oxygen 0.125/ 15.99 X 100 = 44.33 % 3. Number of moles of Magnesium 0.157/ 24.21 = 0.00658 g/mol 4. Number of Moles of Oxygen 0.125/ 15.99 = 0.00782 g/mol 5. Mole ratio 0.00658/ 0.00782 = 0.88 1:0.88 1:1 6. Theoretical Yield (0.157g Mg) (1 mole Mg/ 24.31 g Mg) (1 mole MgO/ 1 mole Mg) (40.3 g Mg/ 1 mole MgO) = 0.26g MgO 7. Percent Yield 0.282 g MgO / 0.26 g MgO X 100= 108.46%
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Summary of Results % Mg in Magnesium Oxide 55.46% % O in Magnesium Oxide 44.33% Mole Ratio Mg: O 1:0.88 1:1 Empirical Formula of Magnesium Oxide MgO Theoretical Yield of Magnesium Oxide 0.26 g MgO % Yield of Magnesium Oxide 108.46% Conclusion The purpose of this lab, to prepare a metal oxide and determine its empirical formula and demonstrate the law of constant composition. The results were then used to find the percent of
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  • Fall '19
  • Magnesium, Oxide, Christina McCool, 0.157g Mg

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