Balancing Chemical Equations Using Oxidation Numbers

Click For Summary
SUMMARY

This discussion focuses on balancing chemical equations using oxidation numbers and half-reaction methods. The user initially struggles with balancing the equation involving Fe(OH)2 and Fe2O3, realizing the need to account for the two iron atoms in Fe2O3. The consensus is to balance the iron first, followed by using intuition and trial and error for the remaining elements. While the oxidation number (ON) method is available, participants recommend the half-reaction method as a more effective approach for complex equations.

PREREQUISITES
  • Understanding of oxidation numbers in redox reactions
  • Familiarity with balancing chemical equations
  • Knowledge of half-reaction method for redox balancing
  • Basic chemistry concepts regarding reactants and products
NEXT STEPS
  • Study the half-reaction method for balancing redox reactions
  • Learn how to apply oxidation numbers in complex chemical equations
  • Practice balancing equations with multiple reactants and products
  • Explore advanced techniques for balancing chemical equations
USEFUL FOR

Chemistry students, educators, and anyone preparing for chemistry exams who seeks to improve their skills in balancing chemical equations and understanding redox reactions.

carlodelmundo
Messages
133
Reaction score
0

Homework Statement



http://carlodm.com/pictures/problem.png

The Attempt at a Solution



I'm stuck. Usually I balance the equation by multiplying the Fe(OH)2 and Fe2O3 by 3. However, I can no longer do this because Fe2O3 has two iron's per one molecule.

Do I multiply one by 6 and the other by 3?
 
Last edited by a moderator:
Physics news on Phys.org
Assume 2Fe(OH)2 is your reagent (why? because Fe2O3 contains two Fe atoms, just keep iron atoms forming one molecule of product togehter) - then you will have to multiply everything by 3. Basically that's the same as multiplitcation by 3 & 6, but it is easier to follow the reasoning.

--
 
I see. So I should balance the reactant iron first, to 2... then do the multiplications of irons by 3.

I've arrived at that step but the products side still looks like a mess. Is this where I stop all "techniques" and rely on intution and trial and error to figure out the balanced equation?
 
Once you have Fe and Cr balanced rest you have to "balance by inspection" - which, as you have correctly pointed out, is a fancy name for "intuition and trial and error" :wink:

Do you have to use ON method?

--
 
No we're not required to use the ON method... but it is a tool that we are able to utilize for ugly equations such as this. Thanks for your help! This'll come handy for reviewing my Chem exam.
 

Similar threads

Chemistry How do we interpret the steps in the algorithm to balance a redox equation?
  • · Replies 7 ·
Replies
7
Views
2K
Oxidation Numbers for H3AsO4 and H2S Equation
  • · Replies 5 ·
Replies
5
Views
2K
Chemistry What is the purpose of redox reactions?
  • · Replies 18 ·
Replies
18
Views
5K
Iron metal reacts with oxygen problem
  • · Replies 2 ·
Replies
2
Views
7K
Using matrices to balance chemical equations
  • · Replies 11 ·
Replies
11
Views
2K
Chemistry How to understand this acidic oxide chemical reaction?
  • · Replies 3 ·
Replies
3
Views
2K
Chemistry Why Do Sulfurous Compounds Show Different Peaks in X-ray Absorption Spectra?
  • · Replies 1 ·
Replies
1
Views
2K
Chemistry How can oxidation numbers be used to balance chemical equations?
  • · Replies 4 ·
Replies
4
Views
2K
Chemistry Understanding chemical potential of gas in mixture versus pure gas, used in derivation of equilibrium constant
  • · Replies 1 ·
Replies
1
Views
2K
What Is the Mass Percent of Iron in the Compound?
  • · Replies 4 ·
Replies
4
Views
5K