Question by Alex: Is there actually a formula for silver oxide like this (Ag5O2), where did i go wrong in my calculations?
I did a lab at school called, Determination of the Empirical Formula of Silver Oxide, we took a sample of silver oxide and heated it with a bunsen burner for some time to drive off the oxygen, leaving the silver metal behind.
In my data table I recorded the mass of the crucible and the the lid in grams (21.268g), the mass of the crucible, lid, and silver oxide (21.842), and the mass of the crucible, lid, and silver metal (21.814). Using the data above, I am supposed to find the mass of silver oxide in grams, the mass of the silver metal produced in grams, the mass of the oxygen produced in grams, percent compositions of silver and oxygen, the moles of oxygen in the silver oxide sample, the moles of silver in the silver oxide sample, the ratio of Ag/O in the silver oxide, and finally the empirical formula of AgxOy.

I calculated the mass of the silver oxide which is 0.574g , the mass of the silver produced which is 0.546g, and the mass of the oxygen which is 0.028. Ive also calculated the percent composition of silver which is 95% and the percent composition of oxygen which is 5%. I've also calculated the moles of oxygen in the silver oxide sample which is rounded to 0.002 mol and the moles of silver which is rounded to 0.005 mol.

This is the part where I think I messed up, my mole ratio came out to be 2.5 to 1 and the empirical formula came out to be Ag5O2. Is this empirical formula actually correct? I know that the formula for silver oxide is Ag2O but my calculations do not match, so please tell me what I did wrong?

Please calculate the masses, percents, moles, the ratio, and the formular again to show me what I did wrong.
Please perform the stoichiometric calculations.

Best answer:

Answer by Cee
formula is ag20

What do you think? Answer below!
[wprebay kw="1+gram+silver+rounds" num="0" ebcat="11116"]
[wprebay kw="1+gram+silver+rounds" num="1" ebcat="11116"]
[wprebay kw="1+gram+silver+rounds" num="2" ebcat="11116"]