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Determining Chemical Formulas

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Introduction

Determining a Chemical Formula Abstract: The purpose of this laboratory is to create a bond between two or more substances to determine the empirical formula of the substance. The bond that is trying to be created in this lab is magnesium oxide. By heating the magnesium and introducing water, will create magnesium oxide which massing the final product and comparing it to the original will produce the values for the empirical formula. Procedure: The procedure was taken from experiment 5 in General Chemistry by Grace R. ...read more.

Middle

6. Heat gently and then strongly with lid slightly displaced for 5 minutes 7. Cool crucible and then weigh. 8. Record your data and calculations Data: The following data table, table 2, was created after the weights were obtained. Weight of the crucible 19.83g Weight of the crucible & Magnesium 20.12g Weight of the Magnesium 0.29g Moles of magnesium 0.011929 0.29g Mg x (1 mol Mg / 24.31g Mg) = 0.011929 moles Weight of the crucible & Magnesium oxide 20.31g Weight of oxygen 0.19g Moles of oxygen 0.011875 0.19g O x (1 mol O /16g O) ...read more.

Conclusion

Analysis: The masses obtained from both the magnesium and the magnesium oxide were reasonable. As evident from Table D, the magnesium had 1.0045 moles which when compared to 1 mole of oxygen, was way less than a 1% error. This resulting indicates that the empirical formula for magnesium oxide is: 2Mg + O2 => 2MgO The ionic bond between one magnesium and one oxygen atom formed magnesium oxide. The compound that was created was a white powder. Conclusion: The formation of a compound was successful. A mol to mol ratio of 1 to 1 was recovered. The empirical formula that was determined in the lab was the correct empirical formula for the creation of magnesium oxide. ?? ?? ?? ?? ...read more.

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