Is 3FeCl2 to 2FeCl3 and Fe(s) a Disproportionation Redox Reaction?

In summary, the given reaction is a redox reaction where ferrous chloride acts as both the oxidizing and reducing agent, resulting in a change in the oxidation number of iron from +2 to +3 and a formation of elemental iron.
  • #1
Elvis 123456789
158
6

Homework Statement


Determine the oxidizing agent, reducing agent, element oxidized, element reduced, # of electrons lost per atom, and # of electrons gained per atom. State if the reaction is not redox.

3FeCl2(aq) ------> 2FeCl3(aq) + Fe(s)

Homework Equations

The Attempt at a Solution


3FeCl2(aq) ------> 2FeCl3(aq) + Fe(s)
+2 -1 +3 -1 0

Those are the oxidation numbers i got. Is this not a redox reaction because only the oxidation number of Fe changes?
 
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  • #2
Elvis 123456789 said:

Homework Statement


Determine the oxidizing agent, reducing agent, element oxidized, element reduced, # of electrons lost per atom, and # of electrons gained per atom. State if the reaction is not redox.

3FeCl2(aq) ------> 2FeCl3(aq) + Fe(s)

Homework Equations

The Attempt at a Solution


3FeCl2(aq) ------> 2FeCl3(aq) + Fe(s)
+2 -1 +3 -1 0

Those are the oxidation numbers i got. Is this not a redox reaction because only the oxidation number of Fe changes?
This is a Redox reaction where ferrous chloride is both the oxidizing agent and the reducing agent. This kind of reaction is called a disproportionation reaction.
 

FAQ: Is 3FeCl2 to 2FeCl3 and Fe(s) a Disproportionation Redox Reaction?

What is a Redox Reaction?

A Redox reaction is a chemical reaction in which the oxidation states of atoms are changed. It involves the transfer of electrons from one molecule to another, resulting in the formation of new chemical compounds.

How do you determine if a reaction is a Redox Reaction?

A reaction is considered a Redox reaction if there is a change in the oxidation states of atoms involved. This can be determined by looking at the charges of the atoms before and after the reaction.

What are some examples of Redox Reactions?

Some common examples of Redox reactions include combustion, rusting, and photosynthesis. In combustion, a substance reacts with oxygen to produce heat and light, resulting in a change in oxidation states. Rusting is a slow Redox reaction in which iron reacts with oxygen to form iron oxide. Photosynthesis is a biological Redox reaction in which plants use sunlight to convert carbon dioxide and water into glucose and oxygen.

What is the importance of Redox Reactions?

Redox reactions are important in many aspects of our daily lives. They are essential for energy production, as they are involved in the process of respiration and photosynthesis. Redox reactions are also used in many industrial processes such as the production of metals and chemicals. Additionally, they play a crucial role in biological processes within our bodies.

How are Redox Reactions balanced?

To balance a Redox reaction, the number of electrons transferred must be equal on both sides of the equation. This can be achieved by adding coefficients and ensuring that the total charge of the reactants is equal to the total charge of the products. It is also important to balance the atoms and charges of each element involved in the reaction.

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