Lab 1: Determination of the Empirical Formula of Silver Oxide

Topics: Mass, Chemistry, Oxygen Pages: 3 (582 words) Published: March 1, 2012
Andy Chen andAlexander Van Buren9/15/11
AP ChemistryDr. Isotone
Lab 1: Determination of the Empirical Formula of Silver Oxide Lab Objective:
In this experiment, the percent composition and empirical formula of silver oxide will be determined. Silver oxide will be heated until it decomposes to silver metal and oxygen, and the percent calculation and empirical formula can be calculated based on combining the ratios of silver and oxygen in the reaction.

Summary of Lab Procedure:
1. Set up Bunsen burner on a ring stand beneath and clay triangle.

2. Adjust height of the clamp so it is 1 cm above the burner

3. Light Bunsen burner and heat the crucible for 1 min, then cool.

4. Weigh the crucible and lid.

5. Measure approximately .5g of silver oxide and weigh.

6. Place crucible in triangle, heat for 2-3 minutes.

7. Heat for an additional 10 minutes.

8. Maximize flame and heat for an additional 10 minutes.

9. Turn off gas and remove burner.

10. Use tongs to remove crucible.

11. Allow to cool on lab bench.

12. Measure combined mass and record on data table.

13. Note appearance of the product and dump into waste container. Pre lab questions #1-4 on separate sheet
Data Tables:
Trial #1
Mass of crucible and lid, g| 30.759 g|
Mass of crucible, lid, and silver oxide, g| 31.387 g|
Mass of crucible, lid, and silver metal, g| 31.344 g|
Appearance of product| White, chalk like|

Trial #2
Mass of crucible and lid, g| 31.300g|
Mass of crucible, lid, and silver oxide, g| 31.734g|
Mass of crucible, lid, and silver metal, g| 31.701g|
Appearance of product| White, chalky|

Trial #1 Trail #2
Mass of AgO| 0.628 g| 0.434 g|
Mass of Ag| 0.585 g| 0.401 g|
Mass of O| 0.043 g| 0.033 g|
% Ag| 93.2%| 92.4%|
% O| 6.8%| 7.6%|
Moles Ag| 0.00542 moles| 0.00402 moles|
Moles O| 0.0027 moles| 0.0021...