Please Explain this reation to me Very Briefly

  • Thread starter Thread starter Maisara-WD
  • Start date Start date
  • Tags Tags
    Explain
Click For Summary

Discussion Overview

The discussion revolves around the reactions of iron (Fe) with oxidizing acids, specifically concentrated sulfuric acid and nitric acid. Participants seek clarification on the chemical processes involved, including the products formed and the underlying thermodynamic principles. The conversation includes both theoretical and practical aspects of these reactions.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested
  • Mathematical reasoning

Main Points Raised

  • Some participants present the reactions of iron with nitric and sulfuric acids, noting the formation of various products, including iron(III) and hydrogen gas.
  • One participant suggests that the reactions are driven by thermodynamics and entropy, indicating that the products have lower energy than the reactants.
  • Another participant challenges the accuracy of the proposed reactions, asserting that nitric acid should produce iron(III) rather than iron(II) and that sulfuric acid's role as an oxidizer is questionable.
  • Concerns are raised about the representation of hydrogen as a product, with some arguing that it would reduce nitrate ions instead.
  • Questions are posed regarding the conditions under which strong oxidizers like nitric and sulfuric acids produce iron(III) and the basis for their reduction to oxides.
  • Participants express uncertainty about the correct stoichiometry and the role of different oxidation states in these reactions.

Areas of Agreement / Disagreement

There is no consensus on the accuracy of the proposed reactions or the roles of the acids involved. Multiple competing views exist regarding the products formed and the mechanisms of oxidation and reduction.

Contextual Notes

Participants note potential typos and misunderstandings in the chemical equations presented. There is also a lack of clarity regarding the thermodynamic principles and redox potentials that govern these reactions.

Who May Find This Useful

This discussion may be of interest to students and educators in chemistry, particularly those exploring redox reactions and the behavior of metals in acidic environments.

Maisara-WD
Messages
18
Reaction score
0
Hi All

Will you please please explain this reaction to me.. Very Briefly??

The reaction of a metal eg. Fe with an oxidizing acid eg. conc sulphuric or dil or conc nitric...

Fe + 4HNO3 -----> Fe(NO3)3 + 2H2O + NO

3Fe + 8H2SO4 ----conc hot-----> Fe(SO4)3 + 4SO2 + 8H2O

Of course passivation occurs with conc Nitric acid.

I need your help to get the whole staff in my mind... I have millions of undescribable questions.. explain and help me please ;)

thanx very very much
 
Chemistry news on Phys.org
Maisara-WD said:
Hi All

Will you please please explain this reaction to me.. Very Briefly??

The reaction of a metal eg. Fe with an oxidizing acid eg. conc sulphuric or dil or conc nitric...

Fe + 4HNO3 -----> Fe(NO3)3 + 2H2O + NO

3Fe + 8H2SO4 ----conc hot-----> Fe(SO4)3 + 4SO2 + 8H2O

Of course passivation occurs with conc Nitric acid.

I need your help to get the whole staff in my mind... I have millions of undescribable estions.. explain and help me please ;)

thanx very very much
Im altering your original reactions for the following explanation
2Fe + 4(HNO3) ---> 2(Fe(NO3)2) + 2H2

2Fe + 4(H2SO4) ---> 2(FeSO4) + 2(SO2) + 4(H2O)

Reactions are driven by thermodynamics and/or by entropy
In the first reaction the nitrate group is preferentially oxidizing the iron and releasing hydrogen. The hydrogen is displaced here since the heat of formation,( the enthalpy change),of iron nitrate is greater than the heat of formation of nitric acid. So the products are in lower energy than the reactants.
For the second reaction Ill just say that the above also applies to the sulphate group ,in terms of preferentially oxidizing the iron with a greater delta H
And there is also an increase in entropy
 
Last edited:
Maisara-WD said:
Will you please please explain this reaction to me.. Very Briefly??

Please elaborate - explain what?

Please note that at least iron(III) sulfate formula is wrong. Can be a typo.

morrobay said:
2Fe + 4(HNO3) ---> 2(Fe(NO3)2) + 2H2

2Fe + 4(H2SO4) ---> 2(FeSO4) + 2(SO2) + 4(H2O)

Both reactions are wrong.

First - no need for some of the parentheses, it is not 4(HNO3) but 4HNO3.

Second - nitric acid is a strong oxidizer, so it will produce Fe(III), not Fe(II). That means also reducing nitric acid to its oxides.

Third - in the reaction with sulfuric acid, if you put SO2 between products, that means you are assuming sulfuric acid acted as an oxidizer. That means iron is oxidized further than to +2, to oxidize it to +2 just H+ is enough.
 
For the first reaction if it was dilute nitric acid and iron then the iron could be Fe ++,
2Fe + 4HNO3 ---> 2Fe(NO3)2 +2H2
For the second reaction with iron and sulfuric acid I would have originally put:
Fe + H2SO4 ---> FeSO4 + H2

correct?
 
Much better now.
 
Can't understand how you write hydrogen as a product in the reaction metal + HNO3: hydrogen reduces immediately NO3- in those conditions.

The correct one is the first written by the OP:

Fe + 4HNO3 -----> Fe(NO3)3 + 2H2O + NO

Furthermore, if HNO3 is very diluted, hydrogen reduces NO3- even to ammonium ion...
 
Borek said:
Second - nitric acid is a strong oxidizer, so it will produce Fe(III), not Fe(II). That means also reducing nitric acid to its oxides.

That's what I do want to understand...

WHY and how the strong oxidizers as conc sulphuric acid or nitric acid produce Fe(III) and not Fe(II)...
And more important: What is the basis on which these oxidizers are reduced into their oxides>>??

thank u all guys..

I'm waiting
 
Maisara-WD said:
WHY and how the strong oxidizers as conc sulphuric acid or nitric acid produce Fe(III) and not Fe(II).

It is all in th eredox potentials.

What is the basis on which these oxidizers are reduced into their oxides>>??

No idea what you are asking about. That's the way the react when they act as oxidizers.
 
lightarrow said:
Can't understand how you write hydrogen as a product in the reaction metal + HNO3: hydrogen reduces immediately NO3- in those conditions.

The correct one is the first written by the OP:

Fe + 4HNO3 -----> Fe(NO3)3 + 2H2O + NO

Furthermore, if HNO3 is very diluted, hydrogen reduces NO3- even to ammonium ion...

OK
Your right. It looks like i took a wrong turn on this.
Not having my 1A, 1B text doesn't help.
 

Similar threads

Calculation could somebody help me please?
  • · Replies 2 ·
Replies
2
Views
4K