9225 g These two values should be equal by the law of conservation of mass. These results do not obey the law of conservation of mass. Possibly she made a mistake recording her numbers. 28. When 31 g of phosphorus reacts with oxygen‚ 71 g of an oxide of phosphorus is the product. What mass of oxygen is needed to produce 13 g of this product? 31g + x = 71g 71g - 31g = 40g oxygen This means that in
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Formula of oxide Na2O2 MgO Al2O3 SiO2 P4O10 Cl2O Melting Point (C) 460 2825 2072 1700 340 -120.6 Boiling Point (C) 657 3600 2977 2230 360 2.2 State at STP Solid Solid Solid Solid Solid Liquid Action of water Dissolve in water and form alkaline solution Slightly dissolve in water and form alkaline solution Insoluble in water Insoluble in water Dissolve in water and form acidic solution Dissolve in water and form acidic solution pH of aqueous solution
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rusting Steel bubbles No reaction No reaction rusting No reaction rusting No reaction Table 2: Observations Results: HCl(Solution used) Metal Word Equation Balanced Equation Cu NR NR Mg Magnesium + Hydrochloric Acid ---> Hydrogen + Magnesium Chloride Mg(s) + 2HCl(aq) ---> H2(g) + MgCl2(s) Sn NR NR Zn NR NR Fe NR NR Steel (FeAl) Iron (III) + Hydrochloric Acid ---> Hydrogen + Iron (III) Chloride 2Fe(s) + 6HCl(aq) ---> 3H2(g) + 2FeCl3(s)
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Table 8.1- Combustion of magnesium ribbon Observations Reaction was exothermic; magnesium ribbon burned and was glowing a bright white color when ignited. Reactants: Mg and O2 Products: MgO Balanced chemical equation 2Mg + O2 2MgO Table 8.2- Combustion of heptane Observations When holding test tube inverted over heptane flame‚ condensation formed against top walls of the test tube. When the burning splint was added the walls of the test tube became less foggy from the condensation
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Semester – CH 2307 TECHNICAL ANALYSIS LAB -2010 INDEX SHEET CYCLE ONE Date of Condn. Date of Subn. Sign 1 Estimation of COD of the given sample of water. 2 Estimation of Manganese in the given pyrolusite ore. 3 Estimation of Magnesium by EDTA method. 4 Estimation of purity of drug using pH meter. 5 Estimation of Ammonia in ammonium salts. 6 Polarimetric estimation of sugar CYCLE TWO Date of Condn. Date of Subn. Sign 7 Estimation of Phosphorous
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apparatus and coming out into the atmosphere. After setting this up‚ researchers continued to crush magnesium turnings into smaller pieces in order to expose fresh metal by removing possible magnesium oxide that was on the surface of the turnings. The turnings were added to the round bottom flask as well as an iodine crystal‚ which facilitates the reaction by cleaning the surface of the magnesium metal. Bromobenzene and anhydrous diethyl ether were then added to the flask. Anhydrous ether was used
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series is a list of metals arranged in order of their reactivity based on displacement reactions‚ reduction of their oxides by hydrogen or carbon‚ the relative ease of decomposition of their compounds and reactions with oxygen‚ dilute acids and water. The higher up a metal is in the reactivity series‚ the more reactive it is. In the experiment conducted‚ the three metals‚ magnesium‚ zinc and copper each had to undergo displacement reactions and reactions with water‚ oxygen and dilute acids‚ to arrange
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Chung-Harris and Mike Taylor Chemistry for CAPE by Susan Maraj and Arnold Samai Periodic Trends in Group II Elements in Group II The elements in Group II are called alkaline earth metals. Be‚ Mg‚ Ca‚ Sr‚ Ba‚ Ra Beryllium‚ Magnesium‚ Calcium‚ Strontium‚ Barium‚ Radium These elements bond by metallic bonds (intramolecular forces) to form giant metallic structures. The size of the atoms increases down the group Physical properties of Group II metals Ionization
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number of moles of hydrogen ions in 100 cm3 of 0.100mol/dm3 hydrochloric acid. (ii) Give an ionic equation to represent the neutralization reaction. Q2. Manganese (IV) oxide catalyses the decomposition of aqueous hydrogen peroxides. In an experiment 50.0 cm3 of aqueous hydrogen peroxide was mixed with 0.50 g of manganese (IV) oxide. The total volume of oxygen formed was measured every 10 seconds. The results of the experiment are shown in the graph. (i) After how many seconds did the
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Hypothesis The hypothesis of this experiment is magnesium oxide can be synthesized by combining (burning) the magnesium with oxygen. The chemical and physical properties of each element (magnesium‚ oxygen‚ and magnesium oxide) might be different‚ from the state‚ color‚ electrical conductivity‚ and pH. Aim This experiment was performed to synthesize magnesium oxide by direct combination of magnesium and oxygen and to compare the properties of the elements (magnesium and oxygen) in their elemental state with
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