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The standard Gibbs energy for the given ...

The standard Gibbs energy for the given cell reaction is `KJmol^(-1)` at 298 K is :
`Zn(s)+CU^(2+) (aq) rightarrow Zn^(2+) (aq) + Cu(s)`
`E^(@)= 2V at 298 K`
(Friday's constant , `F = 96000 C mol^-1`)

A

(-192)

B

(-384)

C

`(192)`

D

384

Text Solution

AI Generated Solution

To find the standard Gibbs energy (ΔG°) for the given cell reaction at 298 K, we can use the relationship between Gibbs energy, the number of moles of electrons transferred (n), Faraday's constant (F), and the standard cell potential (E°). The equation is given by: \[ \Delta G° = -nFE° \] ### Step-by-Step Solution: ...
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