AP Chem Experiment #1 laboratory - determining the Empirical Formula of silver Oxide Materials: Crucible through lid Ring stand with clay pipestem triangle and also ring Bunsen burner Crucible tongs Balance silver oxide sample, 0.5 g Formula: AgxOy (s)  2Ag (s) + O2 (g) Purpose: In this experiment the percent composition and empirical formula of silver oxide will certainly be determined. Silver- oxide decomposes to silver- metal and also oxygen as soon as strongly heated. Heating silver oxide causes the oxygen to be moved off, leaving just the silver steel behind. According to the regulation of conservation of Mass, the total mass that the commodities of a chemistry reaction must equal the fixed of the reactants. In the situation of the decomposition of silver oxide, the complying with equation should be true: massive of silver- oxide = mass of silver steel + fixed of oxygen If both the initial mass of silver- oxide and the final mass the the silver steel are measure, the diminish in mass need to correspond come the massive of oxygen that combined with silver. The percent composition and also empirical formula of silver- oxide deserve to then be calculated, based on combining the ratios that silver and also oxygen in the reaction. The decomposition of silver- oxide right into silver and oxygen gas will use a heat source to rate the decomposition. The experiment is design to enable students to determine the worths of x and y in the formula above. Pre-Lab Questions: A item if iron weighing 85.650 grams was shed in air. The massive of iron oxide developed was 118.370 g. A. Use the molar mass of stole to convert the massive of iron come moles. B. According to the law of conservation of Mass, what is mass of oxygen the reacted through iron and how many moles the oxygen room there in the product? c. Utilizing the moles of iron and moles that oxygen, identify the empirical formula for iron oxide. Note: fountain of atoms do not exist in compounds. In the situation where the proportion of atoms is not a totality number (or really close to a totality number), the proportion of each have to be multiply by a continuous to give whole number rations for all atoms. Procedure: 1. Assemble the ring stand, ring, clay triangle and also Bunsen burner per the example on the former table. 2. Achieve a crucible and also lid. 3. Place the crucible and also lid in the clay triangle every the instance on the front table. 4. Light your Bunsen burner. Gently warm the crucible for around 1 min, then place the Bunsen burner under the crucible and heat the crucible and also lid for an additional 4 minutes. Rotate off the Bunsen burner.5. Permit the crucible to cool on the clay pipestem for about 5 minutes. Then remove it native the clay pipestem and also place that on the wire gauze pad. When the crucible is cool (about 10 minutes), take it the crucible come the digital balance and mass it to the nearest 0.001 g. Record the value in the data table detailed below. 6. Through the lid and crucible quiet on the electronic balance, add enough silver oxide to the crucible such that the overall mass rises at the very least 0.5 grams. Document the worth in the data table. 7. Collection the crucible ago on the clay pipestem. Readjust it for this reason the lid is just off the crucible. Relight the Bunsen burner. Gently warm the crucible and contents because that 2 minutes. Then ar the burner under the crucible for secondary 12 minutes. ~ this time questioning the instructor to assist you in maximizing the flame. Warm the crucible in the many intense part of the flame because that 12 minutes. CAUTION: execute not be breathing the smoke. Execute not skinny over the crucible. Stay about an arm’s length away indigenous the crucible. 8. ~ 12 minutes, revolve off the gas resource and remove the burner. Allow the crucible come cool for a couple of minutes while sitting on the clay triangle 9. Making use of tongs, eliminate the crucible lid and also place it on the cable gauze ~ above the bench top. Through the tongs, remove the crucible native the clay triangle and also place that on the cable gauze. 10. Enable the crucible and contents come cool completely (at least 10 minutes). 11. Measure the an unified mass of the crucible, crucible lid, and also silver metal product. Document the mass in the data table. 12. Dispose the the silver product in the container noted by the instructor. 13. Repeat the experiment utilizing a brand-new sample of silver- oxide. DATA TABLE trial 1Trial 21. Fixed of crucible and also lid, g 2. Massive of crucible, lid, and silver oxide, g 3. Fixed of crucible, lid, and silver metal, g14. Complete the Data results Table Data results Table DT = Data Table entrance 1. Massive of silver oxide, g (DT2 -DT1) 2. Mass of silver, g (DT3-DT1) 3. Fixed of oxygen produced, g (DT2-DT3) 4. % composition of silver- 1 5. % ingredient of oxygen2 6. Moles of O in silver oxide3 7. Moles of silver in silver oxide4 8. Mole ratio5Trial 1Trial 29. % error 10. Empirical formula6 1. 2. 3. 4. 5.% composition = mass of silver divided by fixed of silver- oxide times 100% % composition = fixed of oxygen divided by massive of silver- oxide times 100% mole of O in silver oxide = massive of oxygen divided by 16.00 mole of Ag in silver- oxide = fixed of silver divided by 107.9 division the moles of silver and also the moles of oxygen by the smaller sized of the two numbers. Among the numbers will certainly equal 1. 6. The empirical formula is AgxOy where x and y space the mole ratios derived in 5. Ideally, they room 2 come 1 as the empirical formula is Ag2O (the one is not written). Perform not pressure the answer. If the ratios you obtain are not 2 come 1, that is OK. If the various other number is not close come a totality number, climate multiply both number by a entirety number until both numbers room close come a whole number. For instance – you get 2.5 for one ratio and also 1 for the other. Multiply both by 2 and you gain 5 and 2. These space the subscripts you use to write the empirical formula.

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7. Describe what might have unable to do wrong and how you could improve the procedure/experiment..