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

AI Thread Summary
The reaction 3FeCl2(aq) → 2FeCl3(aq) + Fe(s) is identified as a disproportionation redox reaction. In this process, ferrous chloride acts as both the oxidizing and reducing agent. The oxidation state of iron changes from +2 in FeCl2 to +3 in FeCl3, while elemental iron is produced with an oxidation state of 0. This indicates that iron is both oxidized and reduced during the reaction. Therefore, the reaction qualifies as a redox process due to the change in oxidation states of iron.
Elvis 123456789
Messages
158
Reaction score
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?
 
Physics news on Phys.org
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.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
View full post »

Thread 'Prove that evolution is constant (Provide at least two arguments to support your position)'

I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
View full post »

Similar threads

Chemistry "The oxidized species of the couple is very oxidizing". Does this make sense?
Replies
5
Views
990
Chemistry How do we interpret the steps in the algorithm to balance a redox equation?
Replies
7
Views
2K
Chemistry How to apply Nernst equation in this problem?
Replies
3
Views
2K
Chemistry How to find the pH of a galvanic cell (MIT OCW problem set)
Replies
2
Views
3K
Which Reactions Are Redox?
Replies
2
Views
1K
Redox Reaction in Dissolved Ammonium Chloride
Replies
5
Views
3K
Is Potassium Hydroxide a Reducing Agent in the Reaction with Chlorine?
Replies
1
Views
2K
Number of electrons to balance redox reaction
Replies
5
Views
2K
Fixing a Rusted Snowboard Edge with REDOX Reactions
Replies
1
Views
2K
How to Balance the Oxidation of H2S to Sulfate?
Replies
1
Views
4K

Hot Threads

Recent Insights

Back
Top