Oxidation reaction-which is oxidized?

[alphaj]

Homework Statement

2Ag2S(s) + O2(g) = Ag2O(s) + S(s)

Which is being oxidized?

Homework Equations

N/a

The Attempt at a Solution

Reactants:
Ag2S is neutral, with Ag having +1 charge and S having 2- charge.
O2 is neutral

Products:
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.

 

[Merlin3189]

I agree with your analysis.
Oxidation and reduction are two sides of the same coin, which is why these reactions are often called redox reactions.

When Ag + 2S -> Ag₂S the silver is oxidised from Ag to Ag⁺ and the sulphur reduced from S to S^2-
The silver was already oxidised and did not change. The S^2- was oxidised back to S

 

[Borek]

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+.

Bullseye.

 

[Merlin3189]

So much more concise than me!

 

[alphaj]

Thank you for your help; both of you! I'm relieved that I am thinking about this the right way!