• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Finding the empirical formula of magnesium oxide

Extracts from this document...

Introduction

Mohamad Zulhilmi bin Azmi 930813-05-5385 Chemistry HL ________________ INTRODUCTION Magnesium oxide or magnesia, is a white solid mineral that occurs naturally as periclase and is a source of magnesium. Magnesium oxide is hygroscopic in nature and care must be taken to take it from moisture. Magnesium oxide is easily made by burning magnesium ribbon which oxidises in a bright white light, resulting in a powder. It is formed by an ionic bond between magnesium and oxygen atom in a certain ratio of magnesium to oxygen. Empirical formula is the simplest whole ratio number of all elements present in the compound. It does not express the real composition of a molecule as molecular formula. For instance, the empirical formula of glucose (molecular formula = C6H12O6) is CH2O, and the empirical formula of hydrogen peroxide (molecular formula = H2O2) is HO. An experiment will be carried out to determine the empirical formula of magnesium oxide, you will react elemental magnesium with elemental, atmospheric oxygen, to generate magnesium oxide. Mg(s) + O2(g) ? MgxOy(s) AIM To determine the empirical formula of magnesium oxide HYPOTHESIS Empirical formula of Magnesium oxide is MgO. ...read more.

Middle

It was then placed under the crucible for strong heating while its lid was lifted occasionally. 8. The magnesium was heated strongly until it turned into gray-white powder. 9. Heating was stopped to allow the crucible, lid and contents to cool. 10. The crucible and its lid, and the end product was weighted 11. Step 1 until 11 was repeated for the second experiment. PRECAUTIONARY MEASURES 1. Goggles need to be wear throughout the experiment. This is because the bright flame produced during reaction is hard to distinguish and emits a harmful intensity of UV light 2. Do not breathe the fumes generated. Inhalation of magnesium oxide fumes can cause metal fume fever TABULATION OF DATA 1. Raw data Mass/g (± 0.01g) Experiment 1 Experiment 2 Magnesium, m1 0.30 0.30 Crucible and lid, m2 22.13 22.13 Crucible and lid + magnesium, m3 22.43 22.45 Crucible and lid + product, m4 22.60 22.62 1. Processed data Aspects Experiment 1 Experiment 2 m1/g (± 0.01g) 0.30 0.30 Number of moles, magnesium /mol = 0.0123 = 0.0123 Mass of oxygen, m5 /g (±0.01g) ...read more.

Conclusion

EVALUATION Overall, the experiment produced a reliable results. However, there are small percentage error on the mass of MgO which indicates that are errors on some aspects of the experiment. Firstly, the time for the opening of the lids was too long. When this happened, some of the MgO escaped to the air and resulted in less mass of the MgO. Secondly, the amount of heat supplied was not even throughout the experiment. This was due to the air movement in the laboratory. The presence of air movement has reduced the amount of heat supplied to magnesium. SUGGESTED IMPROVEMENT Some ways can be implemented to improve the accuracy of the result of the experiment so that it will become closer to the theoretical value. The first thing to consider is reducing the time taken for the opening of the lids. We can avoid the escaping of the MgO to the surrounding by using this method. Next, wind shield must be used during the heating of magnesium. An even heating process can be obtained as we prevent the intervention of air movement which will reduce the amount of heat supplied to the magnesium. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Experiment - The Empirical Formula of Magnesium Oxide

    over the Bunsen burner. 7. Periodically lift the lid (using the tongs) to check if the reaction is complete. 8. When the reaction is finished turn off the Bunsen burner and allows the crucible to cool.

  2. Empirical Formula of Magnesium Oxide

    = Trial 2: = = Trial 3: = = Trial 4: = = = = Therefore, the average amount of oxygen obtained throughout the trials was 0.08g�0.02g As a percent uncertainty: % uncertainty of experimental mass of O2 Therefore, the average amount of oxygen obtained throughout the trials was 0.08g�0.02g

  1. Lab Experiment : The change in mass when magnesium burns. (Finding the empirical formula ...

    + 0.0001= 0.3936g (The mass of magnesium ribbon = The mass of the crucible, lid and magnesium- mass of the crucible and lid) 2.Mass of oxygen that combine with Mg ( in grams) +0.0001= 0.2160g (Mass of oxygen = mass of magnesium oxide, crucible, lid - mass of magnesium, crucible, lid)

  2. An Experiment to Determine the Empirical Formula of Lead Iodide

    Approximately 20 cm3 of distilled water was added to each beaker. 8) The solution (beaker #1, 2 and 3) was heated again until it steams. 9) Each beaker was removed from heat. 10) Approximately 1.2 g of potassium iodide (KI)

  1. Finding thr Percentage Composition of Magnesium Oxide

    The mass of the crucible was measured and recorded again, but with the magnesium ribbon inside. A ring clamp was attached to a retort stand and was adjusted so that the flame of the Bunsen burner touched the bottom of the crucible.

  2. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    1 × lab coat The lab coat is used to prevent damages from any spillage of chemicals onto clothing. 1 × covered shoes Covered shoes are needed to prevent any damages to the feet that could be due to spillage of corrosive HCl.

  1. Chemistry Investigation to find the Empirical Formula of Magnesium Oxide

    4 33.979 - 33.834 = 0.145 5 39.264 - 39.113 = 0.131 6 32.823 - 32.784 = 0.039 *Some data has been removed in the following tables due to lack of validity Table 4 - Processed data of the total weight of magnesium and crucible (g)

  2. Discovering the formula of MgO

    use tongs to handle the crucible lid and do not attempt to weigh crucible until it is cool. Procedure: Take 2-3 cm of Magnesium ribbon and observe how it looks. Then using tongs hold it over a Bunsen burner, when it burns hold the magnesium over a little beaker and observe the product formed.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work