# To Determining the empirical formula of MgO

Few research questions that could be used to guide a study To Determining the empirical formula of MgO:

How does the burning temperature of magnesium affect the accuracy of the empirical formula of magnesium oxide?

What are the most common sources of error in determining the empirical formula of magnesium oxide, and how can they be minimized?

How does the purity of the starting materials (magnesium ribbon and oxygen gas) affect the accuracy of the empirical formula of magnesium oxide?

How does the size of the sample of magnesium oxide used to determine the empirical formula affect the accuracy of the results?

Can the empirical formula of magnesium oxide be accurately determined using different methods (such as heating the magnesium oxide in a furnace instead of a Bunsen burner)? If so, how do the results compare?

Materials:

• Magnesium ribbon
• Crucible and lid
• Bunsen burner
• Clay triangle
• Heat-resistant mat
• Balance
• Beaker of water
• Stirring rod
• Filter paper
• Funnel

Instructions:

Begin by setting up the Bunsen burner and clay triangle on the heat-resistant mat.

Place the crucible and lid on the clay triangle, and place the magnesium ribbon inside the crucible.

Light the Bunsen burner and adjust the flame so that it is directed at the bottom of the crucible.

Heat the crucible and magnesium ribbon until the magnesium catches fire and begins to burn.

When the flame goes out and the burning has stopped, carefully remove the crucible from the heat and allow it to cool.

Once the crucible has cooled, weigh it and record the mass.

Place the crucible back on the clay triangle, and heat it until the magnesium oxide begins to glow red.

Once the magnesium oxide has stopped glowing, carefully remove the crucible from the heat and allow it to cool.

Once the crucible has cooled, weigh it and record the mass.

Calculate the mass of the magnesium oxide by subtracting the mass of the empty crucible from the mass of the crucible with the magnesium oxide.

Determine the empirical formula of magnesium oxide by dividing the mass of the magnesium oxide by the atomic mass of magnesium, and then dividing the mass of oxygen by the atomic mass of oxygen.

Combine the number of moles of magnesium and oxygen in the empirical formula to determine the empirical formula of magnesium oxide.

Sample Lab Report:

Title: The Effect of Burning Temperature on the Empirical Formula of Magnesium Oxide

Introduction: The empirical formula of a compound is the simplest whole number ratio of the atoms of each element present in the compound. In this experiment, we will be determining the empirical formula of magnesium oxide, a compound formed when magnesium burns in the presence of oxygen. The burning temperature of the magnesium can affect the accuracy of the empirical formula, as different burning temperatures can lead to different amounts of oxygen being consumed. In this study, we will investigate how the burning temperature of magnesium affects the accuracy of the empirical formula of magnesium oxide.

Methods:

• We obtained a sample of magnesium ribbon and a crucible with a lid.
• We set up a Bunsen burner and a clay triangle on a heat-resistant mat.
• We placed the crucible and lid on the clay triangle, and added the magnesium ribbon to the crucible.
• We lit the Bunsen burner and adjusted the flame so that it was directed at the bottom of the crucible.
• We heated the crucible and magnesium ribbon until the magnesium caught fire and began to burn.
• We allowed the flame to go out and the burning to stop, and then carefully removed the crucible from the heat and allowed it to cool.
• We weighed the crucible and recorded the mass.
• We placed the crucible back on the clay triangle, and heated it until the magnesium oxide began to glow red.
• We allowed the magnesium oxide to stop glowing, and then carefully removed the crucible from the heat and allowed it to cool.
• We weighed the crucible and recorded the mass.
• We calculated the mass of the magnesium oxide by subtracting the mass of the empty crucible from the mass of the crucible with the magnesium oxide.
• We determined the empirical formula of magnesium oxide by dividing the mass of the magnesium oxide by the atomic mass of magnesium, and then dividing the mass of oxygen by the atomic mass of oxygen.
• We combined the number of moles of magnesium and oxygen in the empirical formula to determine the empirical formula of magnesium oxide.

Results: To Determining the empirical formula of MgO:

• The mass of the empty crucible was 22.5 grams.
• The mass of the crucible with the magnesium oxide was 25.0 grams.
• The mass of the magnesium oxide was 2.5 grams.
• The empirical formula of magnesium oxide was determined to be MgO.

Discussion: The results of this experiment indicate that the burning temperature of magnesium does not significantly affect the accuracy of the empirical formula of magnesium oxide. The empirical formula of MgO was obtained consistently, regardless of the burning temperature of the magnesium. This suggests that the burning temperature of the magnesium does not significantly impact the amount of oxygen consumed during the reaction.

Conclusion: In conclusion, this experiment showed that the burning temperature of magnesium does not significantly affect the accuracy of the empirical formula of magnesium oxide. The empirical formula of MgO was obtained consistently, regardless of the burning temperature of the magnesium. Further research could be conducted to investigate other factors that may affect the accuracy of the empirical formula of magnesium oxide.

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