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

Empirical Formula of Magnesium Oxide

Extracts from this document...


Empirical Formula of Magnesium Oxide Name: Suleman Esam Date: 16/10-07 Purpose: The purpose of this lab was to experimentally determine the empirical formula of magnesium oxide. Background: Metal oxide is formed when a metal reacts with oxygen. Magnesium is an alkaline earth metal. When magnesium is heated, it reacts vigorously in the preset of oxygen. It is easy to ignite it when it is shred or powdered, but difficult when it is bulk. Once the metal is ignited, it is hard to extinguish it. Equipments: - Magnesium ribbon - Crucible & lid - Bunsen burner - Steel wool - Pipe clay triangle - Tripod - Crucible tongs - Balance - Goggles Procedure: 1. We took on our goggles and stated the experiment. 2. First we placed a tripod over a Bunsen burner. On the tripod, we placed a pipe clay triangle and over it the crucible & lid. 3. ...read more.


7. Finally, when the magnesium that finished reacting, we let it cool. When it had cooled, we recorded the mass of crucible with magnesium oxide and its lid. COMBINED MASS OF THE OBJECTS AFTER = 33.450g �0.002g Result Now I have every mass that I need to find the empirical formula for magnesium oxide, except the mass of oxygen. By subtracting the mass that the object before the reaction from what it had after magnesium was burned, we find the mass of oxygen. COMBINED MASS OF THE OBJECTS BEFORE - COMBINED MASS OF THE OBJECTS AFTER = MASS OF OXYGEN (33.450g - 33.279g) � (0.002g + 0.002g) = 0.171g �0.004g A summary of all the mass is listed in the chart below. OBJECT MASS (g) UNCERTAINTY (g) Objects before 33.279 �0.002 Objects after 33.450 �0.002 Mg 0.324 �0.002 Oxygen 0.171 �0.004 Magnesium oxide 0.495 �0.006 By finding the amount of moles of these two atoms, we can determine the empirical formula for magnesium oxide. ...read more.


Errors The mole of magnesium and oxygen was not the same. I found out that the mass of oxygen was smaller then it was supposed to be. This error can have occurred by three things: 1. We did not found out the empirical formula for magnesium oxide properly; because magnesium also reacted with nitrogen. It takes three magnesium atoms, while it takes only two nitrogen atoms to form a compound. Nitrogen is also lighter then oxygen; thus our combined mass after the reaction became smaller then if the magnesium had totally reacted with oxygen. 2. When we lifted the lit while magnesium ribbon was reacting, we let out smoke. That was magnesium oxide in vapour. 3. There is a possibility that maybe not all of the magnesium reacted. Improvements: If we had carried the experiment a little more, we could have removed the magnesium nitride. By adding some drops of water and then heating it up, we will get this formula: Mg3N2 + 6H2O � 3Mg(OH)2 + 2NH3 The result will be ammonia gas, which will depart when heated. ?? ?? ?? ?? ...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. Analysis of the Nitrogen Content of Lawn Fertiliser

    + OH-(aq) --> NH3(g) + H2O(l) The basic solution needed for titration was reached through heating the solution to remove the ammonium ions. By heating it, the rate of reaction between the ammonium ions and hydroxide ions increases, consequently producing water and ammonia. Since ammonia is an extremely volatile gas, boiling the solution will result the vaporization rate, which is the desired outcome.

  2. Experiment - The Empirical Formula of Magnesium Oxide

    Once cooled, zero the scales and use the tongs to carefully place the crucible and lid on the scales. Record the mass. 10. Repeat steps 1 - 9 (OR collect results from other groups). Experimental Report Data Collection and Processing Photograph of Lab Setup Photo 1: Laboratory Setup 1.

  1. Empirical Formula of Magnesium Oxide

    or 0.08g�25% Find the average mass of magnesium in the experiment Trial 1: - = = Trial 2: = = Trial 3: = = Trial 4: = = = = Therefore, the average amount of magnesium obtained throughout the trials was 0.2g�0.02g As a percent uncertainty: % uncertainty of experimental

  2. A comparison of various proprieary antacids

    needed to neutralize excess Hydrochloric acid(25 cm3, 0.5 M), after addition of an Eno sachet, for three trials. Trial Number 1 2 3 Final Volume of NaOH, cm3 �0.05 cm3 23.20 20.50 20.60 Initial Volume of NaOH, cm3 �0.05 cm3 0.00 0.00 0.00 Volume of NaOH �0.1 cm3 23.20 20.50

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

    4.Number of moles of oxygen atoms that were used. = 0.0135mole (the number of moles of oxygen = mass / atomic weight . the atomic weight of magnesium is 16.0 g / mole ) 5.Simplest ratio: Mg = 0.0162 Mole = 1.2 0.0135mole Oxygen = 0.0135mole = 1 0.0135mole Multiply by the smallest whole number you can possibly find

  2. Finding thr Percentage Composition of Magnesium Oxide

    The water could have been contaminated. Also, the weighing scale could have been faulted. Recommendations Part B of this investigation was lacking and this caused confusion with the procedure. For future classes, Part B should be added. Also, the Apply & Extend questions should be clearer as they were quite confusing.

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

    From the 6cm strip of Magnesium ribbon, a 3 cm strip was cut and wiped with a clean cloth to remove any contaminants. 4. The 3cm strip of Magnesium was then weighed using the electronic balance. Its mass was noted.

  2. Discovering the formula of MgO

    closest to our theoretical value (40%) and thus has the minimum amount of percentage error. % Error= (| (38.1 - 40)/40 |)*100= 4, 90 % Proving the formula of magnesium oxide: Now in order to prove our results we need to find the formula of magnesium oxide in theory, for

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