AP Chem Experiment #1 lab - identify the Empirical Formula of silver- Oxide Materials: Crucible through lid Ring stand with clay pipestem triangle and 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 be determined. Silver oxide decomposes to silver- metal and oxygen as soon as strongly heated. Heating silver- oxide causes the oxygen to be moved off, leaving just the silver metal behind. According to the regulation of preservation of Mass, the complete mass of the assets of a chemical reaction must equal the mass of the reactants. In the situation of the decomposition of silver oxide, the adhering to equation must be true: mass of silver oxide = massive of silver metal + mass of oxygen If both the initial massive of silver- oxide and also the last mass of the silver steel are measure, the diminish in mass should correspond to the fixed of oxygen that linked with silver. The percent composition and also empirical formula of silver- oxide can then it is in calculated, based on combining the ratios that silver and 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 designed to enable students to identify the values of x and y in the formula above. Pre-Lab Questions: A piece if steel weighing 85.650 grams was shed in air. The fixed of steel oxide created was 118.370 g. A. Use the molar massive of iron to convert the mass of iron to moles. B. Follow to the law of conservation of Mass, what is mass of oxygen the reacted with iron and also how plenty of moles that oxygen are there in the product? c. Making use of the mole of iron and moles that oxygen, identify the empirical formula for iron oxide. Note: fractions of atoms execute not exist in compounds. In the case where the proportion of atom is no a totality number (or really close come a totality number), the proportion of each need to be multiplied by a continuous to give entirety number rations for all atoms. Procedure: 1. Assemble the ring stand, ring, clay triangle and Bunsen burner per the instance on the front table. 2. Obtain a crucible and lid. 3. Place the crucible and lid in the clay triangle per the example on the former table. 4. Light your Bunsen burner. Gently warmth the crucible for about 1 min, then ar the Bunsen burner under the crucible and also heat the crucible and also lid for secondary 4 minutes. Revolve off the Bunsen burner.5. Permit the crucible come cool top top the clay pipestem for around 5 minutes. Then eliminate it indigenous the clay pipestem and place that on the cable gauze pad. Once the crucible is cool (about 10 minutes), take it the crucible to the electronic balance and mass it to the nearest 0.001 g. Record the value in the data table provided below. 6. V the lid and crucible quiet on the digital balance, include enough silver- oxide to the crucible such that the overall mass increases at least 0.5 grams. Record the worth in the data table. 7. Set the crucible back on the clay pipestem. Readjust it for this reason the lid is just off the crucible. Relight the Bunsen burner. Gently warmth the crucible and also contents for 2 minutes. Then ar the burner under the crucible for secondary 12 minutes. After this time asking the instructor to help you in maximizing the flame. Warm the crucible in the most intense component of the flame because that 12 minutes. CAUTION: do not be breathing the smoke. Do not lean over the crucible. Stay about an arm’s size away from the crucible. 8. After ~ 12 minutes, rotate off the gas resource and remove the burner. Enable the crucible to cool for a couple of minutes while sit on the clay triangle 9. Using tongs, eliminate the crucible lid and place it on the wire gauze ~ above the bench top. With the tongs, eliminate the crucible from the clay triangle and place that on the cable gauze. 10. Enable the crucible and contents to cool completely (at the very least 10 minutes). 11. Measure the linked mass the the crucible, crucible lid, and also silver steel product. Record the massive in the data table. 12. Dispose of the silver product in the container provided by the instructor. 13. Repeat the experiment using a new sample of silver- oxide. DATA TABLE psychological 1Trial 21. Fixed of crucible and also lid, g 2. Fixed of crucible, lid, and silver oxide, g 3. Massive of crucible, lid, and also silver metal, g14. Finish the Data outcomes Table Data results Table DT = Data Table entry 1. Fixed of silver oxide, g (DT2 -DT1) 2. Fixed of silver, g (DT3-DT1) 3. Massive of oxygen produced, g (DT2-DT3) 4. % composition of silver- 1 5. % ingredient of oxygen2 6. Moles of O in silver oxide3 7. Mole of silver- in silver- oxide4 8. Mole ratio5Trial 1Trial 29. % error 10. Empirical formula6 1. 2. 3. 4. 5.% composition = massive of silver split by mass of silver oxide time 100% % ingredient = fixed of oxygen divided by fixed of silver- oxide time 100% moles of O in silver- oxide = massive of oxygen separated by 16.00 mole of Ag in silver- oxide = massive of silver divided by 107.9 division the moles of silver and the mole of oxygen by the smaller sized of the two numbers. One of the numbers will equal 1. 6. The empirical formula is AgxOy whereby x and y space the mole ratios derived in 5. Ideally, they space 2 come 1 as the empirical formula is Ag2O (the one is not written). Carry out not force the answer. If the ratios you gain are not 2 to 1, the is OK. If the various other number is no close come a entirety number, then multiply both numbers by a entirety number till both numbers room close to a entirety number. For example – you gain 2.5 because that one ratio and also 1 for the other. Multiply both through 2 and also you obtain 5 and also 2. These space the subscripts you use to create the empirical formula.


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7. Explain what might have gone wrong and how you could improve the procedure/experiment..