Question

How would I do the follow equation? What are the steps?

Identify and write the (unbalanced) oxidation and reduction half-reactions for the following reactions.

(a) Solid copper dissolves in an acidic solution containing nitrate ions to form copper (II) ions and nitrogen dioxide gas.

(b) Solid zinc dissolves in hydrochloric acid to form zinc ions (+2 charge) in solution and hydrogen gas.

(c) Solid iron (III) oxide reacts with solid carbon to produce solid iron and and gaseous carbon dioxide.

Answer 1

(a) first write the information as Cuis) & Nog (aq) + + Now, write the oxidation No. on each +2 Cu(s) + Nght Cut & gren + (ap) + No la Species +4 No +5 Decrease in oxidation NO. - Reduction. Increase in oxidation No. = oxidation oxidation Cul Cult (cor) Reduction: Noz (92) — NO(g)

16) Given Zn(s) + Hella) write oxidation Number: Zn²+ (aq) + H2 (97 +1 -1 En & na - 2 + H Decrease in oxidadon No. - Reduction, Increase in oxidation No. = oxidation oxidation Zn - Zn. Reduction : ut 2 2+ only itt is getting reduced, co is a Spectator lon, which don't get into redox reaction +3 - 2 & (s) + & (s) – Fe(s) + Colg) +4-2 (C) Increase Decrease oxidation. Reduction : c. 1s) - Fe (5) Ca (g) Fe(s)
we just have to find the oxidation number of each species undergoing redox to identify oxidation and reduction.