1 Determine the Amount of Oxygen that is Thermally...

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1 Determine the Amount of Oxygen that is Thermally Decomposed from a Predetermined Mass of Potassium Chlorate INSTRUCTOR: Sunday, February 08, 2015 PURPOSE/INTRODUCTION

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2 The purpose of this experiment is to theoretically and experimentally calculate the amount of oxygen that is thermally decomposed from a predetermined mass of potassium chlorate(s). The mass percentages of the elements within the compound will be calculated using the molar masses as well as the chemical formula of the compound. Followed by a practical experiment using a 10g sample of potassium chlorate(s) and heating it to a point where all of the oxygen is decomposed into potassium chloride(s) and oxygen(g). MATERIALS Materials required to test the hypothesis in a lab include: 10g sample of potassium chlorate Test tube Bunsen burner
METHOD Part One: Calculate mass percent of potassium and chlorine within the potassium chlorate compound. Using the Periodic Table of Elements determine the molar mass of potassium chlorate by taking the sum of the molar masses of potassium 39.0983, chlorine 35.453, and oxygen 15.9994*3. Once the GMW (gram-molecular-weight) of potassium chlorate is determined. Molar mass of KClO3 = atomic mass of K + Cl + O 3 = 39.0983 + 35.453 + 15.9994*3 = 39.0983 + 35.453 + 47.9982 = 122.5495 g/mol Calculate the mass percent of each element. Mass percent of potassium(s) = Molar Mass of P Molar Massof KClO 3 X 100 = 39.0983 122.5495 X 100 = 0.31904 X 100 = 31.904% Mass percent of chlorine(s) = Molar Mass of Cl Molar Mass of KClO 3 X 100 = 35.453 122.5495 X 100 = 0.28929 X 100 = 28.930% Part Two: Calculate the theoretical mass percent of oxygen that will be thermally decomposed from the 10g sample of potassium chlorate(s) using the molar masses of both oxygen(g) O=15.9994 and potassium chlorate(s) KClO 3 =122.5495. As well as

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