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Determination of a Formula by Analysis Principle: Determine the percent of Silver and Oxygen in Silver Oxide to determine the empirical formula. Experimental Procedure: Place a clean porcelain crucible without lid onto a wire triangle on a tripod or ring. Heat the crucible for several minutes to a dull red heat using the hottest blue flame that the Bunsen burner will produce. Allow crucible to cool to room temperature then weigh it on an analytical balance to the nearest 0. 001 g.
Handle the crucible only with forceps and carry it in a clean, dry beaker. Cover the crucible with all of the Silver Oxide and weigh precisely again. Heat crucible until there is no further change that can be observed. Repeat the process again until a constant weight is obtained, signifying the reaction is complete. Raw Data: Weight of crucible + silver oxide = 18. 178 g Weight of empty crucible = 16. 884 g Weight of silver oxide = 1. 294 g Weight of AgO + crucible after heating = 18. 085 g Weight of after second heating = 18. 075 g Weight of silver = 1. 191 g Weight of oxygen = 0. 103 g Calculations: Take the weight of the silver and divide by the weight of silver oxide and multiply by 100 to find the percent of silver in silver oxide. 1. 191 gAg/ 1. 294 g AgO 100 % = 92. 0 % of Ag in AgO Repeat with the oxygen. 0. 103 gO 2 / 1. 294 g AgO 100 % = 8. 0 % of O 2 in AgO Derive the formula of silver oxide. 92 gAg/ 107 gAg = 0. 8598 mol Ag 8 gO/ 16 O = 0. 50 mol O 0. 8598 mol Ag/ 0. 50 mol O = 1. 719 0. 50 mol O/ 0. 50 mol O = 1 Ag 1. 719 O 1 The empirical formula for silver oxide is Ag 2 O. The balanced equation: 2 Ag 2 O? 4 Ag + O 2 Answers and Questions: Do not heat with yellow flame at any time.
Why? Because heating with a yellow flame will cause soot to form at the bottom of the crucible.
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