Determination Of The Empirical Formula Of Silver Oxide
Melissa Carrithers
9-17-14
Period: 6
Determination of the Empirical Formula of Silver Oxide
Purpose:
To find the percent composition and empirical formula of silver oxide can then be calculated, based on combining the ratios of silver and oxygen in the reaction.
Hypothesis:
Silver oxide decomposes to silver metal and oxygen when strongly heated. Heating Silver oxide causes the oxygen to be driven off, leaving only the silver metal behind. The total mass of the products of a chemical reaction must equal the mass of the reactants.
Mass of silver oxide = Mass of silver metal + Mass of oxygen
The initial mass of silver oxide subtracted by the mass of silver metal corresponds with the mass of oxygen.
Procedure:
1. Weigh the mass of the crucible, and lid then weigh out 0.5g of silver oxide with crucible and lid.
2. Put the crucible with silver oxide in the clay triangle, and light Bunsen burner.
3. Brush the bottom of the crucible with the Bunsen burner for 2-3 minutes and than for 10 minutes. Let cool for 10 minutes
4. Clean
Determining Silver Oxide
Trial 1
Trial 2
Trial 3
Mass of crucible, and lid, g.
Mass of crucible, lid, and silver oxide, g.
Mass of crucible, lid, and silver metal, g.
Appearance of product
Data Table:
X______________________________________________________
Conclusion:
The Empirical Formula for Silver Oxide is Ag2O. The percent composition ratio was 2:1. According to my data, the hypothesis is correct. Mass of silver oxide = Mass of silver metal + Mass of Oxygen although each trial varied with answers. When decomposing Silver Oxide to form Silver Metal and Oxygen the balanced equation is 2Ag2O → 4Ag + O2.
Discussion:
If the balance equation needs four moles of Ag than does that meant the molecular formula is Ag4O2? Also, confused about how to find the percent yield and as to why it may be lower or higher than 100% because of the mass of the product weighing more than the theoretical mass.
9-17-14
Period: 6
Determination of the Empirical Formula of Silver Oxide
Purpose:
To find the percent composition and empirical formula of silver oxide can then be calculated, based on combining the ratios of silver and oxygen in the reaction.
Hypothesis:
Silver oxide decomposes to silver metal and oxygen when strongly heated. Heating Silver oxide causes the oxygen to be driven off, leaving only the silver metal behind. The total mass of the products of a chemical reaction must equal the mass of the reactants.
Mass of silver oxide = Mass of silver metal + Mass of oxygen
The initial mass of silver oxide subtracted by the mass of silver metal corresponds with the mass of oxygen.
Procedure:
1. Weigh the mass of the crucible, and lid then weigh out 0.5g of silver oxide with crucible and lid.
2. Put the crucible with silver oxide in the clay triangle, and light Bunsen burner.
3. Brush the bottom of the crucible with the Bunsen burner for 2-3 minutes and than for 10 minutes. Let cool for 10 minutes
4. Clean
Determining Silver Oxide
Trial 1
Trial 2
Trial 3
Mass of crucible, and lid, g.
Mass of crucible, lid, and silver oxide, g.
Mass of crucible, lid, and silver metal, g.
Appearance of product
Data Table:
X______________________________________________________
Conclusion:
The Empirical Formula for Silver Oxide is Ag2O. The percent composition ratio was 2:1. According to my data, the hypothesis is correct. Mass of silver oxide = Mass of silver metal + Mass of Oxygen although each trial varied with answers. When decomposing Silver Oxide to form Silver Metal and Oxygen the balanced equation is 2Ag2O → 4Ag + O2.
Discussion:
If the balance equation needs four moles of Ag than does that meant the molecular formula is Ag4O2? Also, confused about how to find the percent yield and as to why it may be lower or higher than 100% because of the mass of the product weighing more than the theoretical mass.