How to Balance Atoms in Ion-Electron Method?

AI Thread Summary
The discussion focuses on the ion-electron method for balancing redox reactions, specifically addressing challenges in balancing two partial equations: H2PO2 to H2PO3^-1 and Fe(OH)3 to Fe(OH)2. The user expresses confusion about balancing oxygen and hydrogen atoms, mentioning the addition of 2OH and H2O but finding it ineffective. There is a request for guidance on how to approach balancing these half-reactions correctly. The conversation emphasizes the importance of correctly applying the steps in the ion-electron method to achieve balanced equations. Clear instructions and examples are sought to resolve the balancing issues presented.
Aafia
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In ion electron method to balance equation we have to follow steps ... i am doing it but here i am confusing how to do this ...
There are two partial equations i have made in basic medium
1- H2PO2---------> H2PO3^-1
2-Fe(OH)3---------->Fe(OH)2
Now the second step is to balance the atoms
By adding 2OH for Oxygen and H2O for Hydrogen
But it can't solve
Helpp me pleasezzzz
Thanks
 
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Show how you approach the first reaction.
 
Borek said:
Show how you approach the first reaction.
I had a full reaction
H2PO2+Fe(OH)3------->H2PO3^-1+Fe(OH)2
Then i split it into two partial equations according to rule ..
 
Show how you are trying to balance first (or second, whichever you like) half reaction.
 
Second
 
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...
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