Question

Ni2+ (aq) + Cu(s) ⟶ Ni(s) + Cu2+(aq) Fe(s) + Zn2+ (aq) ⟶ Fe2+ (aq) + Zn (s) ΔSsys = - 15 J/K, DS = + 5 J/K Al(s) + Zn2+ (aq) ⟶ Al3+ (aq) + Zn (s) ΔH = +25 kJ, DS = +100 J/K, T = 300 K

Answer 1

Explanation:

Given the redox reaction

Fe3++V2+→Fe2++V3+

which species is oxidized? Which is reduced? Identify the reducing agent and the oxidizing agent.

Solution

Fe3+ is reduced into Fe2+ and V2+ is oxidized into V3+ . This is because the oxidized species loses electrons, and the reduced species gains electrons.

Iron gains an electron

Fe3+→Fe2+

and vanadium loses an electron

V2+→V3+.

Thus, Fe3+ is the oxidizing agent and V2+ is the reducing agent.