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2.5 Question9 What is the formula of the predicted product from heating magnesium metal and nitrogen...
A. Empirical Formula of Magnesium Oxide mass of crucible and cover + magnesium metal (before heating) 42.36 & 42.11 e 005 0 mass of crucible and cover 46.28 46.05. 011! 46.31 . 10 mass of magneſium metal mass of crucible and cover + magnesium oxide (after heating ) 42.49 & 0 bbb 10 0 mass of combined oxygen (after heating - before heating) w the calculation of the empirical formula for trial I (see Example Exercise 1).
mass of magnesium metal??
Determine the empirical formula of Magnesium Oxide from following data. Show your calculations. Mass of Crucible and Cover + magnesium ribbon (before heating) 27.60 g Mass of crucible and Cover = 27.30 g Mass of magnesium metal = Mass of crucible and cover + magnesium oxide (after heating) = 27.80 Mass of combined oxide (after heating - before heating) =
Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is 2 Mg(s)+O2(g) 2 MgO(s) Consider that you react 12.62 g Mg with 13.08 g O2 gas. What is the theoretical yield of MgO that can be generated from this reaction? Enter a numerical answer only to three significant figures, in terms of grams.
Empirical formula of Magnesium oxide (5 marks) Mass of crucible and cover + magnesium (before heating) 23.4190 g Mass of crucible and cover 23.2950 g Mass of magnesium Mass of crucible and cover + magnesium oxide (after heating) 23.4900 g Mass of oxygen N.B. show calculations
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2Mg(s)+O2(g)→2MgO(s) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 13.1 g of MgO are collected. -Determine the limiting reactant for the reaction. -Determine the theoretical yield for the reaction. -Determine percent yield for the reaction.
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2Mg(s)+O2(g)→2MgO(s) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 13.9 g of MgO are collected. a) Determine the limiting reactant for the reaction. b) Determine the theoretical yield for the reaction. c) Determine percent yield for the reaction.
14. The reaction of magnesium metal with hydrochloric acid produces hydrogen gas as a product. I would like to collect 125 mL of hydrogen gas from the experiment. The temperature of the lab is 23.5°C and the pressure is 762 mmHg. How many grams of magnesium metal should I use if the hydrochloric acid is kept in excess? Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)
3) Solid magnesium and nitrogen gas combine to form solid magnesium nitride. a. Write the balanced chemical equation for this reaction. b. How many grams of magnesium nitride can be produced from the reaction of 10.0 g of magnesium and 12.0 g of nitrogen? c. What is the percent yield for this reaction if 7.159 g of magnesium nitride are isolated following the reaction?
Reaction 1: Magnesium metal in strong acid. Give a description of the reaction: What is the gas produced and what is the source of the gas? Is the production of gas in this reaction an oxidation or reduction? Explain. What happened to the solid magnesium metal during the reaction? Is the change in the magnesium metal you observed an oxidation or Explain reduction? Reducing Agent Oxidizing Agent
96. Magnesium is a very active metal that can be Oxidized with oxygen to MgO nitrogen to MgN2, water to Mg(OH)2 and CO2 to MgO. Write the redox reaction associated With each 0f these four oxidations. As a result of these Processes a Magnesium fire ?s particularly hazardous. Explain why water or cO2 fire extinguisher should not be used with a magnesium fire. How would you extinguish a magnesium fire?