Electrochem! Calculate Eo for the following reaction (posted in comment). Hint: Derive Eo values for the half-reactions in which Ag2S is reduced to Ag metal and Ag(OH)3 is reduced to Al metal. You can do this by combining the standard reaction potentials for reduction of Ag+ (0.7996 V) and Al3+ (-1.662 V) with the Ksp expressions and values of Ag2S (Ksp = 1.6*10^-49) and Al(OH)3 (Ksp = 1.9*10^-33).

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jaredstone4 · Answer

Any and all help is appreciated! I really just don't see how to use the Ksp values to find the given quantity...

parthkohli · Answer

As someone who'll study electrochemistry later this year... is there any relationship between the equilibrium constant and E0 values?

jaredstone4 · Answer

I believe they're related by the Nernst equation... So is Ksp basically Kc? Ksp just refers to solubility in particular while Kc is for general equilibrium?

jfraser · Answer

$E^0$ and $K_{SP}$ values are linked through thermo. You can use $\Delta G$ to equate both of them.

jfraser · Answer

you should be able to use the 2 $K_{SP}$ values to find the concentrations of the ions and then plug them into the nernst equation, yes

jaredstone4 · Answer

Are they linked with the equation $$\Delta G^o=-RTlnK$$ where K is Ksp(prod)/Ksp(react)? Then the given $$\Delta G$$ can be put into $$\Delta G = -nFE^o$$ to solve for $$E^o$$

jfraser · Answer

that's how I would do it

jaredstone4 · Answer

Well, unless I made an algebra error, that didn't work. It still says the answer is incorrect.

jfraser · Answer

I'd have to spend some time with it, but that's the approach I would use

likeabossssssss · Answer

plz close this question wen u r done with it