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The effects of temperature on rates of reaction
The effect of temperature on rate of reaction
The effects of temperature on rates of reaction
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Easha Naik Megan Reiff, Emily Netterville Block 4 21 September 2016 Magnesium Oxide Production Lab Purpose: In this experiment ,you precisely weigh a sample of magnesium metal, and then heat the sample in the air. Magnesium metal reacts with the oxygen (O2) of the air to form Magnesium Oxide (MgO2). 2Mg + O2 2 MgO [Synthesis] After the magnesium sample has reacted completely, the magnesium oxide product is determined. From these two masses, the percentage composition of the magnesium oxide is to be calculated. Data/Results: Parameters Measures •Mass of crucible and cover 27.88 grams •Mass of crucible, cover and magnesium 28.80 grams •Mass of magnesium 0.92 grams •Mass …show more content…
•Mass of oxygen 0.54 grams Calculations: •Mass of magnesium ribbon = Mass of crucible, cover and magnesium ribbon - Mass of crucible and cover = 28.80 g - 27.88 g = 0.92 g •Mass of the magnesium oxide produced = Mass of crucible, cover and magnesium oxide - Mass of crucible and cover = 29.36 g - 27.88 g = 1.48 g MgO •Mass of oxygen reacted with magnesium = Mass of magnesium oxide - Mass of magnesium = 1.48 g - 0.92 g = 0.56 g O •Percent of magnesium in magnesium oxide = MgO = 24.3 g + 16 g = 40.3 g/mol % of Mg = 24.3g10040.3 g/mol= 60.3 % •Percent of oxygen in magnesium oxide = MgO = 24.3 g + 16 g = 40.3 g/mol % of O = 16 g10040.3 g/mol = 39.7 % •Empirical formula of magnesium and oxygen = Mg O 60 g 40 g 60 g24 g/mol 40 g16 g/mol = 2.5 mol 2.5 mol 2.5 mol2.5 mol 2.5 mol2.5 mol = 1 1 MgO •Molecular formula of the compound magnesium oxide 0.92 g Mg1 mol Mg24 g Mg= 0.03833333 mol 0.56 g O 1 mol O16 g O= 0.035 mol (both have the same ratios, its 1) = MgO
The mass of Mg + the mass of O2=mass of MgxOx. Knowing the mass of
magnesium is flammable especially if in powder form, but we are using it in a ribbon form and we are not using any flames in any part of the experiment. The gas which is given off from the reaction between Hydrochloric acid and Magnesium ribbon is Hydrogen which is a flammable gas.
The experimental ratio by mass for magnesium and oxygen in magnesium oxide would be 3:2.
The primary problem that would occur if magnesium were to be substituted by carbon is that carbon and oxygen form the compound CO2 when they react, which is in a gaseous state above -78.5 degrees Celsius, which is far below the temperature at which the experiment was performed. In this state, it is difficult to contain carbon dioxide gas without an airtight container. This experiment is not possible with an airtight container, since oxygen must enter to react with the carbon, and therefore some the carbon dioxide would inevitably escape, rendering the results invalid.
Ø The length of the magnesium ribbon will have to be kept to 0.03g on
The purpose of the lab was to determine the empirical formula of a compound (magnesium oxide). In order to calculate the empirical formula, the mass of each element in the compound was determined. Then, the number of moles of each element in the sample was calculated. Finally, the molar ratio of each element as the smallest whole number was expressed, yielding the compounds empirical formula. The expected empirical formula of Magnesium Oxide was a 1:1 ratio.
Reaction 2: H = 50 x 4.18 x -10.3" H = -2152.7 This value is for 1.37g of calcium oxide, not 56.1g, which is its relative molecular mass. Therefore: H =
Mass of O = Mass of crucible, cover, KClO3 and MnO2 after heating (Step # 11) - Mass of crucible, cover, KClO3 and MnO2 before heating (Step # 5)
Magnesium, also known as atomic number 12 was discovered in 1808 by Sir Humphry Davy who was a British Chemist best known for his experiments in electro-chemistry and his invention of a miner's safety lamp (BBC News, 2014). Magnesium is a chemical element with symbol Mg. Magnesium is a light, fairly strong, whitish, silver Alkaline Earth Metal that is the eighth most abundant element in the Earth's Mantle and the fourth most common element on earth, making up 13% of the planet's mass (Winter, 2011). Its atomic weight is 24.305.
Magnesium is found in large amounts throughout our bodies. We obtain it predominantly from dietary sources. We can also obtain magnesium in many other places since it is the seventh most prevalent element from our universe. The earth’s crust contains large amounts of this element and we can obtain it from the minerals dolomite and carnallite. It is, however, most commonly extracted from our ocean waters.
These discrepancies could have been caused by unyielding chemical reactions that took place. The magnesium had to be heated in the presence of air for approximately 2 minutes to ensure it bonded with nitrogen. Throughout the lab, heating the contents was a problem due to the wind and having the Bunsen burner turned down too low causing the crucible to turn black from the weak flame charring it. Because of this, the magnesium most likely did not have enough time and heat to react with the nitrogen
Investigating the Effect of Varying Concentration on the Reaction between Magnesium Ribbon and Hydrochloric Acid
RMM of citric acid as 210g and I have been told that one mole of
is θ to PO. The downward force by the mass is mg so towards O it will