Natural Sciences

Examples of Redox Reactions

You may be wondering what are Redox reactions and what are the easiest examples of them, for your convenience, we have prepared this article, so that together with us you can learn more about the examples of Redox Reactions.

What are Redox Reactions?

We also know them as oxidation-reduction reactions or reduction-oxidation reactions, these are the chemical reactions that occur through the exchange of electrons through atoms or molecules. This is manifested by the oxidation changes of the reactants.

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The reagent that allows electrons undergoes an oxidation state and the one that absorbs undergoes a reduction state. Oxidation is the predisposition of an atom to take electrons as part of a chemical reaction, we can also define this as valences or oxidation numbers.

Characteristics of Redox Reactions

Like the rest of the chemical reactions, Redox reactions have a series of characteristics that make them different from the rest, below we will list some of them:

  • They occasionally consist of released energy.
  • In general, the results of these tend to be different from the initial compounds.
  • It is comprised of half reactions.
  • These involve perpetual changes in the chemicals of the materials.

Examples of Redox Reactions

Below we will provide you with the most effective examples of Redox reactions:

  1. Fe2O3 + 3CO → 2 Fe + 3 CO2

Reduction or contraction : Fe goes from an oxidation state of +3 to a state of 0, therefore, it undergoes a reduction or contraction.

Oxidation : the C goes from +2 to +4 so we can say that it undergoes an oxidation state.

  1. Zn + AgNO3 → Zn (NO3) 2 + Ag

Reduction or contraction: In this case Ag goes from an oxidation state of + 1 to one of 0

Oxidation : In this case Zn goes from a 0 oxidation state to a +2 state

  • Semi-feedback:

Zn → Zn + 2 + 2e-

2 Ag + + 2e- → 2Ag

  • Integral reaction:

Zn + 2 Ag + + 2e- → Zn + 2 + 2Ag + 2e-

  • Precise reaction:

Zn + 2 AgNO3 → Zn (NO3) 2 + 2Ag

  1. Iron has two forms of oxidation.
  • Iron (II) oxide: FeO.
  • Iron (III) oxide Fe.
  1. The iron (III) ion can be reduced to iron (II):
  • Fe 3+ + 1e  = Fe 2+
  1. Manganese (II) reacts with sodium bismuthate.
  • Mn 2+ (aq) + BiO  (s) = Bi 3+ (aq) + MnO  (aq) + MnO  (aq)
  • Oxidation State: Mn 2+ (aq) = MnO  (aq) + 5e 
  • Reduction or contraction: 2e  + BiO  (s) = Bi 3+ (aq)

Subsequently, the hydroniums must be added and with these, the water molecules where hydrogens are required and oxygen is needed.

  • Oxidation State: 4 H 2 O + Mn2 + (aq) = MnO 4- (aq) + 8H + (aq) + 5e 
  • Reduction or contraction : 2e  + 6H + + BiO 3- (s) = Bi 3+ (aq) + 3H 2 O

These reactions or effects will fluctuate to match the total number of electrons involved, which is obtained by multiplying the half reaction by the number of electrons in the other half reaction so that the sum of electrons is integer.

  • Oxidation state : (4H 2 O + Mn 2+ (aq) = MnO  (aq) + 8H + (aq) + 5e  ) x2
  • Reduction or contraction: (2e  + 6H + + BiO  (s) = Bi 3+ (aq) + 3H 2 O) X5

We will obtain a final result of:

  • Oxidation state: 8H 2 O + 2Mn 2+ (aq) = 2MnO  (aq) + 16H + (aq) + 10e 
  • Reduction or contraction: 10e  + 30H + + 5BiO  (s) = 5Bi 3+ (aq) + 15H 2 O

After providing you with the best information, we invite you to inquire more about this topic and discover other types of chemical reactions and their functions in everyday life.

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