Chapter 19, Problem 19.103QP

Interpretation Introduction

Interpretation:

Balanced equations for oxidation of Iron (II) hydroxide by Oxygen should be written.

Concept introduction:

Balanced equation:

If the chemical equation contains the equal number of atoms and charge in both reactant and product side is known as balanced equation.

Oxidation- Reduction Equations:

In chemical reaction, a chemical species, which loses its electron to gets oxidized and simultaneously another species gains this lost electron gets reduced is known as oxidation- reduction reaction or Redox reaction.

Half reactions:

In the redox reaction split into two half reactions one is oxidation and another one is reduction.

In oxidation half reaction, a chemical species, which lose its electron to get oxidized.

In reduction half reaction, a chemical species, which gains the electron from solution to gets reduced.

Balanced Oxidation- Reduction Equation:

In the oxidation- reduction contains the equal number of atoms and charge in both reactant and a product side is known as balanced oxidation- reduction equation.

• Basic medium redox reaction:

  Two half reactions are written separately then the balance all elements except hydrogen and oxygen.

${\text{H}}^{\text{+}}$ Ions are eliminated by the addition of ${\text{OH}}^{\text{-}}$ ions in both sides.

In the reaction, Charges are balanced by the addition electrons.

If necessary, the two reactions are multiplied by integer and add these balanced two half reactions and remove the spectator species to give a balanced equation of redox reaction.