Determination of the Empirical Silver Oxide Formula Essay Example

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 the 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 of silver oxide and weigh.
6. Place crucible in a triangle, heat for 2-3 minutes.
7. Heat for an additional 10 minutes.
8. Maximize flame and heat for an additional 10 minutes.

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i>Turn off gas and remove the burner.

Use tongs to remove the crucible.

Allow cooling on the lab bench.

Measure combined mass and record on the data table.

Note the appearance of the product and dump it into a waste container.

Measurements of silver oxide Ag2O -> (4) Ag(s) + (1) O2 (g)

The source of error that might account for the higher percent yield could be a measurement error, since putting too much Ag2O could affect the outcome of the experiment by increasing the time needed to heat.

Another error could be the heating time since the product might have been heated for too long or too short.

Conclusion: The present composition of a compound tells us which elements are present in the compound and their mass ratio. Since all the atoms of a given element in a compound have the same average atomic mass, the elements that ar

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