Electrolytic vs Galvanic Cells

[aclementine]

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What's the difference in how you calculate electric potential in these two types of cells?

Also, what's the difference between these two equations:
EMF = E(cathode) - E(anode)
EMF = E(reduction) + E(oxidation)

What if an electrolytic cell is discharging would it act as a galvanic cell?

How do u guys approach these sorta questions in general? I trying to get a better handle on them

 

[Genie133]

What's the difference in how you calculate electric potential in these two types of cells?

Also, what's the difference between these two equations:
EMF = E(cathode) - E(anode)
EMF = E(reduction) + E(oxidation)

What if an electrolytic cell is discharging would it act as a galvanic cell?

How do u guys approach these sorta questions in general? I trying to get a better handle on them

i'm going with omyss' explanation...

 

[Omyss]

EMF=E(cathode)- E(anode), remember that E(anode) will be negative because it'll have a negative reduction potential, so it basically comes out to be the same thing.

not sure about the second part (about electrolytic cell discharging).... but when I do those questions I just try to think of it in terms of reduction potential... if it wants to reduce, it'll have a positive reduction potential, if it wants to oxidize then it's reduction potential is negative

i hope i don't have this backwards...

actually the Eanode will not a lwaysbe negatve.... basically the first equation invoves only the reduction potentials so you take the more positive one and make it the cathode and the less postivie is the anode and you subtract them.

The second one, the more positive is still ther cathode, but the less favourable half reaction is reversed (so the signs change) to make it a oxidation (anode) reaction. Then you add them.

 

[Corpus Callosum]

What's the difference in how you calculate electric potential in these two types of cells?

Also, what's the difference between these two equations:
EMF = E(cathode) - E(anode)
EMF = E(reduction) + E(oxidation)

What if an electrolytic cell is discharging would it act as a galvanic cell?

How do u guys approach these sorta questions in general? I trying to get a better handle on them

There is only one equation you need to remember, and not even if you understand what is going on:
E= E cathode - E anode where reduction takes place at cathode and oxidation at anode.
as for the sign of the equation, you use the standard reduction potentials from the table if given, keeping in mind that the one with greater + potential will be reduced (spontanous, galvanic), so the other one has to be oxidized.
When you are looking at reduction potentials you don't change the sign, just use the equation as is.
Now if you are given two equations, it is simpler, just figure out which is oxidation, and which is reduction and just add the equations.
You don't have to memorize anything, just think

"If you can find a thread of logic in what you are learning, you can always avoid a great deal of pure memorization" Corpus,

 

[Foghorn]

What's the difference in how you calculate electric potential in these two types of cells?

Also, what's the difference between these two equations:
EMF = E(cathode) - E(anode)
EMF = E(reduction) + E(oxidation)

What if an electrolytic cell is discharging would it act as a galvanic cell?

How do u guys approach these sorta questions in general? I trying to get a better handle on them

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