Essay on Silver Oxide Lab
Determination of the Empirical Formula of Silver Oxide
9/12 – 9/13
The purpose of this lab is to use one of the ways to identify different compounds and be able to tell them apart. Based off of experimentation, the empirical formula of the given silver oxide will be determined.
Silver Oxide, 0.5g
Balance, 0.001-g or 0.0001-g precision
Clay pipestem triangle
Crucible and cubicle lid, 15- or 30-mL
Ring stand and ring clamp
Wire gauze with ceramic center
Pre Lab Questions
1. Use molar mass of iron to convert the mass of iron to moles.
85.65g/55.9g 1.534 moles of Iron were used
2. …show more content…
.137/.551 = 25% is the percent composition of oxygen
3. Use the molar mass of silver and oxygen to calculate the moles of each product. Enter the results in the data Results table.
4. 0.137g/ 16.00g = 8.562 E -3
0.413g/ 108.0g = 3.824 E -3
About a 2 to 1 ratio Ag2O
5. Write a balanced chemical equation for the decomposition of the silver oxide to form silver metal and oxygen. 2Ag2O > 4Ag + O2 .
6. The theoretical yield of a product in a chemical reaction is the maximum mass of a product that can be obtained , assuming 100% conversion of the reactant. Calculate the theoretical yield of silver metal in the experiment. .55Ag2O x 1mole/231.74g x 4 mole Ag/2 mole Ag2O x 107.87 = .4654g of silver is the theoretical yield.
7. Use the following equation to calculate the percent yield of silver metal produced in the experiment. .413g of silver / .465g of silver x 100 = 88% is the percent yield.
8. Discuss source error in this experiment that might account for a percent yield lower or higher than 100%. Be specific.
• the balances could have been off
• Not putting in exactly 0.5g of silver oxide
• not putting the crucible under the fire for the right amount of time
• crucible could have absorbed too much water
• not using the right amount of heat
Mass of silver oxide
Mass of silver metal produced