Unit 13b: Applications of Inorganic Chemistry
Introduction:
Within my assignment, I will thoroughly explain the concepts of oxidation and reduction in terms of
electrodes, including the key principles and underlying mechanisms. I will also compose balanced
half-equations and redox equations, and apply these to perform a variety of calculations.
Additionally, I will write a comprehensive experimental report for the three given cells, detailing the
methods and results of the experiments. Finally, I will analyse and evaluate the practical applications
of redox reactions in industrial settings, including their use in analytical procedures.
Oxidation and reduction
Oxidation and reduction are two halves of a chemical reaction in which electrons are transferred
between molecules or atoms. Oxidation is the process by which a molecule or atom loses electrons,
and reduction is the process by which a molecule or atom gains electrons. In a redox (reduction-
oxidation) reaction, the substance that loses electrons is said to be oxidized, and the substance that
gains electrons is said to be reduced. In other words, oxidation is the loss of electrons and reduction
is the gain of electrons.
Half-equations are used to represent the separate oxidation and reduction reactions that occur in a
redox reaction. In a half-equation, the species being oxidized (or reduced) is shown on the left side
of the equation, with the electrons being gained (or lost) indicated on the right side.
A redox equation is the combination of two half-equations, one representing the oxidation and the
other the reduction. A redox reaction can be balanced by using the technique of ion-electron
method (also called half-reaction method)
For example, the redox reaction between zinc and copper ions in solution can be represented by the
following half-equations: Zn(s) → Zn2+(aq) + 2e- oxidation Cu2+(aq) + 2e- → Cu(s) reduction
When the above half-equations are combined, the redox equation is: Zn(s) + Cu2+(aq) → Zn2+(aq) +
Cu(s)
In calculations of redox reactions, the standard electrode potential of the half-reaction are used to
calculate the overall cell potential.
Half equations and redox equations for:
- Zn(s) | Zn^2+ (aq) ¦¦ Cu^2+ (aq) | Cu(s)
Oxidation half equation= Zn(s) ⇌ Zn^2+ (aq) 2^e-
Reduction half equation= Cu^2+(aq) + 2^e- ⇌ Cu(s)
,Full redox equation= Zn(s) + Cu^(2+)(aq) ⇌ Zn^2+(aq) + Cu(s)
- Zn(s) | Zn^+2 (aq) ¦¦ Fe^+2 (aq) | Fe(s)
Oxidation half equation= Zn(s) ⇌ Zn^2+(aq) + 2^e-
Reduction half equation= Fe^+2(aq) + 2^e- ⇌ Fe(s)
Full redox equation= Zn(s) + Fe^+2(aq) ⇌ Zn^2+(aq) + Fe(s)
- Fe(s) | Fe^+2(aq) ¦¦ Cu^+2(aq) | Cu(s)
Oxidation half equation= Fe(s) ⇌ Fe^2+ (aq) + 2^e-
Reduction half equation= Cu^2+ (aq) + 2^e- ⇌ Cu(s)
Full redox equation= Fe(s) + Cu^2+ ⇌ Fe^2+ + Cu(s)
Redox reactions, which involve the transfer of electrons from one molecule or atom to another, are
commonly used in various analytical procedures and industrial processes. In titrations, a solution of
known concentration, called the titrant, is added to a solution of unknown concentration until the
reaction is complete. This allows the concentration of a specific species in the unknown solution to
be determined.
In industrial processes, redox reactions are used in electroplating, where metal ions are reduced to
form a metallic coating on a surface, and in the manufacturing of batteries, where chemical
reactions involving the transfer of electrons are used to store and release electrical energy.
Additionally Redox reactions also used in the production of fertilizers, refining of metals and in many
chemical synthesis and production processes.
Measuring cell potentials
Aim
The purpose of this experiment is to construct three electrochemical cells, and to measure the
potential difference between the electrodes, noting the polarity.
Diagram
, Equipment
Voltmeter, high resistance
3 x Measuring cylinders (20cm3)
Filter paper strips
3 x connecting leads with crocodile clips
4 x beakers (50 cm3)
Goggles
Saturated potassium nitrate solution KNO3
Emery paper (3 small pieces)
Strip of iron wire
Strip of zinc wire
Lead (II) nitrate solution 0.1 M
Strip of copper wire
Zinc sulphate solution 0.1 M
Copper(II) sulphate solution 0.1 M
Ferrous sulphate FeSO4
Safety warnings:
Introduction:
Within my assignment, I will thoroughly explain the concepts of oxidation and reduction in terms of
electrodes, including the key principles and underlying mechanisms. I will also compose balanced
half-equations and redox equations, and apply these to perform a variety of calculations.
Additionally, I will write a comprehensive experimental report for the three given cells, detailing the
methods and results of the experiments. Finally, I will analyse and evaluate the practical applications
of redox reactions in industrial settings, including their use in analytical procedures.
Oxidation and reduction
Oxidation and reduction are two halves of a chemical reaction in which electrons are transferred
between molecules or atoms. Oxidation is the process by which a molecule or atom loses electrons,
and reduction is the process by which a molecule or atom gains electrons. In a redox (reduction-
oxidation) reaction, the substance that loses electrons is said to be oxidized, and the substance that
gains electrons is said to be reduced. In other words, oxidation is the loss of electrons and reduction
is the gain of electrons.
Half-equations are used to represent the separate oxidation and reduction reactions that occur in a
redox reaction. In a half-equation, the species being oxidized (or reduced) is shown on the left side
of the equation, with the electrons being gained (or lost) indicated on the right side.
A redox equation is the combination of two half-equations, one representing the oxidation and the
other the reduction. A redox reaction can be balanced by using the technique of ion-electron
method (also called half-reaction method)
For example, the redox reaction between zinc and copper ions in solution can be represented by the
following half-equations: Zn(s) → Zn2+(aq) + 2e- oxidation Cu2+(aq) + 2e- → Cu(s) reduction
When the above half-equations are combined, the redox equation is: Zn(s) + Cu2+(aq) → Zn2+(aq) +
Cu(s)
In calculations of redox reactions, the standard electrode potential of the half-reaction are used to
calculate the overall cell potential.
Half equations and redox equations for:
- Zn(s) | Zn^2+ (aq) ¦¦ Cu^2+ (aq) | Cu(s)
Oxidation half equation= Zn(s) ⇌ Zn^2+ (aq) 2^e-
Reduction half equation= Cu^2+(aq) + 2^e- ⇌ Cu(s)
,Full redox equation= Zn(s) + Cu^(2+)(aq) ⇌ Zn^2+(aq) + Cu(s)
- Zn(s) | Zn^+2 (aq) ¦¦ Fe^+2 (aq) | Fe(s)
Oxidation half equation= Zn(s) ⇌ Zn^2+(aq) + 2^e-
Reduction half equation= Fe^+2(aq) + 2^e- ⇌ Fe(s)
Full redox equation= Zn(s) + Fe^+2(aq) ⇌ Zn^2+(aq) + Fe(s)
- Fe(s) | Fe^+2(aq) ¦¦ Cu^+2(aq) | Cu(s)
Oxidation half equation= Fe(s) ⇌ Fe^2+ (aq) + 2^e-
Reduction half equation= Cu^2+ (aq) + 2^e- ⇌ Cu(s)
Full redox equation= Fe(s) + Cu^2+ ⇌ Fe^2+ + Cu(s)
Redox reactions, which involve the transfer of electrons from one molecule or atom to another, are
commonly used in various analytical procedures and industrial processes. In titrations, a solution of
known concentration, called the titrant, is added to a solution of unknown concentration until the
reaction is complete. This allows the concentration of a specific species in the unknown solution to
be determined.
In industrial processes, redox reactions are used in electroplating, where metal ions are reduced to
form a metallic coating on a surface, and in the manufacturing of batteries, where chemical
reactions involving the transfer of electrons are used to store and release electrical energy.
Additionally Redox reactions also used in the production of fertilizers, refining of metals and in many
chemical synthesis and production processes.
Measuring cell potentials
Aim
The purpose of this experiment is to construct three electrochemical cells, and to measure the
potential difference between the electrodes, noting the polarity.
Diagram
, Equipment
Voltmeter, high resistance
3 x Measuring cylinders (20cm3)
Filter paper strips
3 x connecting leads with crocodile clips
4 x beakers (50 cm3)
Goggles
Saturated potassium nitrate solution KNO3
Emery paper (3 small pieces)
Strip of iron wire
Strip of zinc wire
Lead (II) nitrate solution 0.1 M
Strip of copper wire
Zinc sulphate solution 0.1 M
Copper(II) sulphate solution 0.1 M
Ferrous sulphate FeSO4
Safety warnings:
