Empirical Formula of Magnesium Oxide Chemistry Tutorial Want chemistry games, drills, tests and more? The total mass of the products of a reaction must equal the total mass of the reactants. Do not look into the crucible when it is heating. Experimental Report Data Collection and Processing Photograph of Lab Setup Photo 1: Laboratory Setup 1. There was no percentage uncertainties involved in molar mass. Suppose you heat one sample of magnesium in pure oxygen so that it is completely converted to magnesium oxide with no worries about magnesium nitride being present.
However, it should be noted that some magnesium oxide will probably be lost as the fine powder quickly escapes from the crucible before the lid is positioned. Experimental Notes Equipment List Caution: Eye protection is essential. The quantitative stoichiometric relationships governing mass and amount is used in the following experiment regarding the combustion reaction of magnesium metal. The ratio of atoms is the same as the ratio of moles. Clean the crucible and repeat the experiment once. This experiment could be furthured by doing it again except with other compounds.
The empirical formula of magnesium oxide was deduced. Formula of a Compound I: Magnesium and Oxygen Overview In this experiment, you precisely weigh a sample of magnesium metal, and then heat the sample in the air. The small amount of nitride that forms can be removed with the addition of water, which converts the nitride to magnesium hydroxide and ammonia gas. In conclusion, the empirical formula of magnesium oxide can be calculated by the known; yet the accuracy may be affected by circumstances, such as the completion of the reaction. Magnesium Mole ratio is in a decimal number of 2.
The masses recorded on Page 33 in Section I, part c include the mass of the containers the mass of the empty containers is recorded in Section I, part b. It was observed that some of the products white powder left on the lid. All three of the trials yielded different results in the data table; but, there were only two different empirical formulas… 1359 Words 6 Pages this lab was to find the empirical formula of magnesium oxide. In this experiment, you will synthesize zinc iodide and determine its empirical formula. The concept of stoichiometry mole equation leads to finding the empirical formula of magnesium oxide.
The gas was turned on again and the Bunsen burner was ignited to a red flame air hole fully open. When the reaction is finished turn off the Bunsen burner and allows the crucible to cool. The masses that were resulted were then used to calculate the empirical formula of magnesium oxide. A crucible and Bunsen burner will be used to heat magnesium metal for burning. The dependant variable will be the mass of Magnesium Oxide, this is a measured variable as the mass of oxygen can be calculated and will enable us to determine the formula for Magnesium Oxide. The Empirical Formula of Magnesium Oxide Essay Sample Experimental Design Focus Question What is the empirical formula for magnesium oxide? If time is limited, it is possible to light the magnesium strip inside the crucible and quickly position the lid using tongs before heating the crucible. Burning magnesium Inhalation Ensure that the room is well ventilated.
Do not breathe the fumes generated. The molar mass is taken to be the relative atomic mass of an element which is the average mass of atoms present in any naturally occurring element relative to the mass of one atom of carbon-12 isotope taken as exactly 12 which gives formula weight sum of the atomic weights of the atomic species as given in the stated formula for the compound. Osmosis is used throughout the kitchen in various countries. Note that oxygen atoms are found in MgO individually…. Then divide through by the smallest number of moles to get a ratio.
All three of the trials yielded different results in the data table; but, there were only two different empirical formulas… 1359 Words 6 Pages this lab was to find the empirical formula of magnesium oxide. The empirical formula is largely useful in determining the ratio of elements within ionic compounds where the structure is of a non-directional nature of bonding where any ion at any time could be surrounded by 4, 6, or 8 oppositely charged ions. Convert the masses into moles dividing by atomic weight in grams. A scatter graph was drawn to show the compositions of magnesium and oxygen within magnesium oxide. Heat the crucible and magnesium, only occasionally lift the lid to let air flow through until magnesium is fully reacted, then remove lid and heat for another minute.
Jillian Hughes, Chemistry Period 6, Beaureguard If the experiment is done correctly then we will be able to accurately calculate the empirical formula of magnesium oxide. Consider an experiment in which 0. The masses of the pure compound and the calcium oxide are measured. From there, you calculate the ratios of different types of atoms in the compound. This creates a pattern of endlessly repeating lattice of ions they do not exist as a free unit of atoms but in crystal lattices with repeating ions in specific ratios which is why empirical formula is used as a form of identification for defining an ionic-bonded substance.
Magnesium metal reacts with the oxygen O 2 of the air to form magnesium oxide. Limitations of Experimental Design Generally, the experiment went well since both qualitative and quantitative data had been produced. The mass would then be heavier than it was weighed. The purpose of firing the crucible at a high temperature was to quickly eradicate any stubborn chemicals which may have resisted cleaning by water, as well as any moisture the crucible may hold to provide a clean and dry equipment which can ensure accuracy and validity of calculations of masses. When zinc and hydrochloric acid are mixed together, the reaction took place in an evaporating dish that was accompanied by hydrogen gas.
You need to become an! Remove the crucible and let it cool before adding a few drops of water to decompose nay nitrides that may have been formed. Moles of oxygen reacted The number of moles of oxygen atoms contained in 0. Express the ratio of moles of each element as small whole numbers. To work out the empirical formula, the value of moles of the different atoms in a compound is needed. From this point on, I like to summarize the calculations in a table. This experiment could be furthured by doing it again except with other compounds. Nevertheless, the theoretical empirical formula of magnesium oxide is MgO.