Magnesium is 24 and oxygen is 16. Do not touch the apparatus, during the experiment it may still be which further can lead to burns. Water contains oxygen, this oxygen would be calculated into the composition of MgO. Mass of magnesium oxide Dependent Variable The mass of this product will be measured after it has been observed that no further reaction will occur. Method: Risk Assessment: What is a risk? One 8cm strip of magnesium ribbon 11. Reaction When magnesium is in its metal form it will burn very easily in air. Magnesium is one of the alkaline-earth metals, and is one of the most common elements in the Earth's crust.
Design: The following figure represents the experiments lab setup, visualize the equipment used. This is known as heating to incandescence. The ratio of atoms is the same as the ratio of moles. This would lead us to calculate a negative number for the amount of magnesium oxide. Solution The empirical formula is the simplest whole-number ratio of atoms in a compound. In its pure form, it is silvery white, and relatively soft, like ash.
Another objective was determining the formula of the compound that results when Magnesium and Oxygen react. Twist it into a loose coil. Another discrepancy that may have occurred during the experiment was that the magnesium strip may have reacted with the oxygen in the air before it was poured into the calorimeter. Place magnesium ribbon into crucible, replace the lid and weigh once more 6. Place the crucible with the substance in it on top of the triangle pipe stem. Aim To work out the molecular formula of Magnesium Oxide. A synthesis reaction is when at least two or more substances combine to form a single product.
Having some Mg3N2 in the crucible as product, instead of pure MgO d. Theory: The purpose of this lab was to confirm the chemical formula of magnesium oxide by comparing the masses of pure magnesium solid prior to any reaction and magnesium oxide solid after a reaction between all of the magnesium and oxygen from the air when heated from a Bunsen burner in a crucible. Continue to heat until lead starts to change to an ash color, lead should start turning very bright 7. Considering this obvious advantage I forego the stomach bloating issue and never thought one of my health supplement magnesium oxide is causing the issue. Then divide through by the smallest number of moles to get a ratio. The reaction is violent but safe, provided the procedure is followed exactly.
If a different lid rather than the experimenting lid was taken to be weighed, then the results would be inaccurate because the lids have different masses. This would contribute to the inaccuracy of the results. So in my experiment we combusted Magnesium ribbon to form Magnesium oxide. Convert the masses into moles dividing by atomic weight in grams. Oxygen and magnesium combine in a chemical reaction to form this compound.
Weigh the crucible along with the Mg ashes, 16. If you have to walk with the crucible to the balance, hold the crucible in the tongs and support it with a heat resistant mat under it to take it to the balance for weighing. Which in this case would be MgO. An expected percent composition, by mass, was found and compared to our experimental results. The final value was the greatest percentage errors in Table 2. How to reduce the risk? Thank you all Hi Udaya - As noted in the Answer, magnesium supplements can cause stomach upset and other symptoms -- and some forms of magnesium may be more likely to cause these effects than others. Planning A: Refer to lab handout entitled, Heat of Reaction for the Formation of Magnesium Oxide.
However, this would explain the small error in this experiment as the discrepancies were not that high. Procedure a Protect the bench with a large sheet of hardboard or heat resistant mats. An exothermic reaction is a term that describes a chemical reaction in which there is a net release of energy heat. Ensure students are wearing eye protection throughout the demonstration. Once again, the change that would have occurred would have been minimal as it is difficult for large amounts of magnesium to react with oxygen in such a short amount of time without the use of a catalyst. There would be too less of oxygen.
Variables Variables identified Type of variable Treatment Amount of magnesium used Independent variable Different groups will use different masses. It burns in air with a brilliant white light, as seen in the experiment, and for this reason is often used in flares and fireworks. Laboratory Investigation: Magnesium Burning Introduction: This experiment introduces stoichiometry, the science of finding out how much stuff is necessary in a chemical equation. W eigh the cru cible, cr ucible li d and the obtaine d magnesi um and recor d respect ive weigh ts. They should divide mass by the atomic mass for each element.
All students plot their masses of magnesium and oxygen onto the graph. Add the mixture to the crucible. Make sure there is only one set of each apparatus so that two pieces of the same apparatus will not be mistaken. The flame provided a source of heat which prompted a chemical reaction to proceed. So now I had the mass of starting magnesium and magnesium oxide. Magnesium hydroxide milk of magnesia and magnesium citrate, for example, are commonly found in over-the-counter products to treat constipation. How is it a risk? Lid-lifting causing loss of mass of the products Random error Lift the lid every 3 minutes instead of irregular time intervals to ensure the reaction taking place thoroughly.