Determination of a Formula by Analysis Determine the percent of Silver and Oxygen in Silver Oxide to determine the empirical formula. 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 0.001g. 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 = 18.178gWeight of empty crucible = 16.884gWeight of silver oxide = 1.294gWeight of AgO + crucible after heating = 18.085gWeight of after second heating = 18.075gWeight of silver = 1.191gWeight of oxygen = 0.103gCalculations: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.1.191gAg/1.294gAgO * 100% = 92.0% of Ag in AgORepeat with the oxygen.0.103gO2/1.294gAgO *100% = 8.0% of O2 in AgODerive the formula of silver oxide.92gAg/107gAg = 0.8598 mol Ag8gO/16O = 0.50 mol O0.8598 mol Ag/0.50 mol O = 1.7190.50 mol O/0.50 mol O = 1Ag1.719O1The empirical formula for silver oxide is Ag2O.The balanced equation: 2Ag2O 4Ag + O2Answers 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....
