Question

Balance the following redox equation, identifying the element oxidized and the element reduced. Show all of the work used to solve the problem.

Ag + CN- + O2 -> Ag(CN)2- + H2O

Pretty lost on this question. This is how I've balanced the equation:
4H+ + Ag + 2CN- + O2 -> Ag(CN)2- + 2H2O

And I don't really know which elements have been oxidized or reduced :/ please help

Answer 1

if someone could just tell me if i balanced it right, i think i could figure out which was oxidized and which was reduced by myself

Answer 2

Yes.

Answer 3

is Ag reduced?

Answer 4

no wait, O is reduced... so which is oxidized?

Answer 5

Remember: \(\sf \color{red}{OIL~RIG}\)
\(\sf \color{red}{O}\)xidation \(\sf \color{red}{I}\)nvolves \(\sf \color{red}{L}\)oss of \(electrons\)
\(\sf \color{red}{R}\)eduction \(\sf \color{red}{I}\)nvolves \(\sf \color{red}{G}\)ain of \(electrons\)

Answer 6

so O isn't reduced? i'm so confused. could you explain please? :/ i'm sorry

Answer 7

What's the oxidation of oxygen on the left?

Answer 8

0 and then on the right, it's -2. so that's why i thought it was reduced

Answer 9

So, it's gained electrons, meaning...

Answer 10

but i thought if the oxidation number decreased, then it was reduced