iron + copper (II) sulfate

Question

a small piece of iron into a test tube containing 1-2 ml of 1.0 M copper (II) sulfate solution



1.) What is the complete balanced equation?

2.) What are the oxidation numbers?

3.) What are the half reactions?

4.) What substance was oxidized? What substance was reduced?

Answer 1

1.) Fe(s) + CuSO₄(aq) ==> FeSO₄(aq) + Cu(s)

2.) Fe(s) = 0; Cu = +2; S = +6; O = -2 .......... Fe = +2; S = +6; O = -2; Cu = 0

3.) Fe ==> Fe²⁺ + 2e- oxidation half reaction

Cu²⁺ + 2e- ==> Cu(s) reduction half reaction

4.) Fe is oxidized and Cu²⁺ is reduced