Question

Part B: Basic Conditions Using the half-reaction method, balance the following redox reactions under basic conditions and identify which of the reactants is being reduced and which is being oxidized. 7. SO32- + Cu(OH)2 → S022- + Cu(OH) a. Oxidized: b. Reduced: c. Balanced Equation: 8. O2 + Mn(OH)2 → MnO2 a. Oxidized: b. Reduced: c. Balanced Equation: 9. NO;' + H2 → NO a. Oxidized: b. Reduced: c. Balanced Equation:

Answer 1

Ans Part B ;

To balance the redox reaction we start by writing the oxidation and reduction half reactions seperately.

Then all the elements are balanced except hydrogen and oxygen . Then oxygen and hydrogen are balanced by adding water and hydrogen ions respectively. The Hydrogen ions are balanced by adding hydroxide ions. The charges are balanced by adding electrons.

The half reactions are then added and simplified to get the balanced redox reactions.

7)

a) Oxidised : SO₃^2-

b) Reduced : Cu(OH)₂

c) Balanced equation :

SO₃^2- + 2Cu(OH)₂ = SO₄^2- + 2Cu(OH) + H₂O

8)

a) oxidised : Mn(OH)₂

b) Reduced : O₂

c) Balanced equation :

O₂ + 2Mn(OH)₂ = 2MnO₂ + 2H₂O

9)

a) oxidised : H₂

b) Reduced : NO₃^-

c) Balanced equation :

2NO₃^- + 3H₂ = 2NO + 2H₂O + 2OH^-