How can we determine if a reaction is reversible or not?

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To determine if a reaction is reversible, the entire balanced equation must be considered, not just a half-reaction. The discussion centers on the zinc-copper redox reaction, which is presented as Cu2+(aq) + Zn(s) -> Cu(s) + Zn2+(aq). While redox reactions are often irreversible, they can become reversible under specific conditions, such as the application of a reverse potential in rechargeable batteries. In this case, the zinc-copper reaction is deemed irreversible as presented. Understanding the full context of the reaction is crucial for accurate assessment.
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how can we determine if a reaction is reversible or not?

Zn2+ (aq) + 2e- -> Zn(s)
is this a reversible reaction?

thanks! :biggrin:
 
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That's not even a reaction... it's only a half reaction! Where did the electrons come from? The entire reaction must be shown to answer the question.
 
oops.. this is the full reaction, it's the zinc-copper cell redox reaction.

Cu2+(aq) + Zn(s) -> Cu(s) + Zn2+(aq)
 
Aren't redox reactions always irreversible?
 
They can be reversible if a reverse potential is applied as in rechargeable batteries. As shown, it is not reversible.
 
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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