Balancing redox equations in acidic solutions

I’m pretty tired right now so I’m not thinking very clearly so this is probably stupidly simple, but I’ve got a bit of a hangup on a question I’m doing.

I’m suppposed to balance this equation assuming it’s in an acid solution (in the presence of H+ ions)

2CuS(s) + HNO3 --> Cu(NO3)2 + H20 + NO (g) + S (s)

Ordinarily I’d balance the half reactions (excluding H and O), add H20 to compensate for O, H+ to compensate for H, and electrons to compensate for charge. But this equation already seems half done. The H2O has been accounted for, etc.

I tried just straight up balancing the equation but it’s sort of unruly. Trying to break it apart into the half reactions also gave me troubles. Any ideas?

EDIT: Forgot to put in the sulphur on the right side of the equation, it’s there now though.

Sulfur doesn’t appear on the left side so, unless you are the creator, this is impossible to balance.

3 Cu (s) + 8 HNO3(aq) 3 Cu(NO3)2(aq) + 4 H2O + 2 NO (g)

( I googled it without the sulfur)


Thanks for the reply, I forgot to add a sulphur but it’s there now.

Anyone out there that can help explain this question to me? I’ve got a few similar to this.

Sorry, but I’m math and science retarded.