AP Chem help please!!!!!! redox rxns

got this question completely wrong on an AP Chem test, but i can do corrections, i just need to be able to explain how i found the answer. But i am so confused. I think i mixed up oxidizing and reducing.

The following reaction takes place in acidic solution:
FeS (s) + NO3- (aq) ----> NO (g) + SO4 2- (aq) + Fe 2+ (aq)

a. ID the element oxidized
b. ID the reducing agent
c. Write the balanced oxidation half-reaction (he made it clear afterwards that only the oxidation one is necessary)

Thanks in advance :)

FeS with Fe at +2 does not change --> Fe 2+ (aq)


FeS with S at -2 ----> gets oxidized to--> SO4 2- (aq) with S at +6 & loses 8 electrons
NO3- with N at +5 takes 3 electrons ----> and gets reduced down to --> NO with N at +2


which simplifies to
oxidation: FeS --> SO4 2- & 8 e-
reduction: NO3- & 3 e- ----> NO

balances electrons as
oxidation: 3FeS --> 3 SO4 2- & 24 e-
reduction: 8 NO3- & 24 e- ----> 8 NO

giving us
3FeS & 8 NO3- --> 3 SO4 2- & 8 NO

adding in the Fe released
3FeS & 8 (NO3) - --> 3 (SO4)-2 & 8 NO & 3 (Fe)+2

add water to balance O's
3FeS & 8 (NO3) - --> 3 (SO4)-2 & 8 NO & 3 (Fe)+2 & 4 H2O

add H+ to balance H's
3FeS & 8 (NO3) - & 8 H+ --> 3 (SO4)-2 & 8 NO & 3 (Fe)+2 & 4 H2O

that's balanced,
(even the charges balance from side to side)


(NO3)-1 is the oxidizing agent
the FeS is the reducing agent