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Nernst equation gives the variation of p...

Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is
`E=E^(@) -(2.303RT)/(nF) logQ (or) E=E^@ - (0.0591)/(n) log Q `
`E^@`= Standard potential and 'Q' is the reaction quotient.
Which cell has least potential ?

A

`ZN// underset(1M)(Zn^(+2))// underset(1M)(Cu^(+2))//Cu`

B

`Zn// underset(0.1M)(Zn^(+2))// // underset(0.1M)(Cu^(+2))// Cu`

C

`Zn // underset(0.1M)(Zn^(+2))// underset(1M)(Cu^(+2))// Cu`

D

`Zn// underset(1M)(Zn^(+2))// underset(0.1M)(Cu^(+2))// Cu`

Text Solution

Verified by Experts

The correct Answer is:
D
`E_("cell") = E_("cell")^(0) + (0.0591)/(n) log "([Cu^(+2)])/([Zn^(+2)])`
` [Cu^(+2)] uarr E_("cell") uarr `
` [Cu^(+2)] darr E_("cell")darr`
Metallurgy , Refer Ellingham Diagram
According to this graph lower line metal reduce upper line metal
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