Why is bubble present, in this redox reaction?

AI Thread Summary
Bubbles formed during the redox reaction between magnesium and iron in a yellow solution are likely due to the release of oxygen gas as magnesium oxidizes. The brown substance observed is probably iron oxide, commonly known as rust, resulting from the reaction between iron and oxygen in the presence of water. The net ionic equation indicates that magnesium is oxidized while oxygen is reduced, leading to the formation of hydroxide ions. The presence of bubbles suggests that gas is being produced, which aligns with the oxidation-reduction process occurring. Understanding these reactions helps clarify the chemical changes taking place in the experiment.
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Homework Statement


In the lab, i saw that when Mg(s) attach with Fe(s) nail in a yellow solution( probably indicator), after one day, the brown substance and bubble are formed.
My net ionic equation is
SOA: O2(g) +2H2O(l) +4e -->4OH-
SRA: Mg(s) --> Mg2+ +2e
NIE: O2(g) +2H2O(l) +2Mg(s)-->4OH- +2Mg2+
Can anyone explain why is bubble formed? and what is the brown substance?(is it MgO or Mg(OH)2, or Fe something??)
Thanks

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The Attempt at a Solution

 
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I immagine it might simply be iron oxide... rust
 
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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