2Ag2S(s) + O2(g) = Ag2O(s) + S(s)
Which is being oxidized?
The Attempt at a Solution
Ag2S is neutral, with Ag having +1 charge and S having 2- charge.
O2 is neutral
Ag2O is neutral, with Ag having a 1+ charge and O having -2 charge.
S is neutral.
So: Reactants and products have the same net charge?
But, S when from 2- to 0 charge. Therefore, it was oxidized (gained two electrons).
Oxygen went form 0 to 2-. So, it was reduced.
Ag stayed the same. 1+ to 1+.
But, I read that Ag is actually being oxidized.
I'm not really sure what's happening.