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For a Ag -Zn button cell , net reaction ...

For a Ag -Zn button cell , net reaction is `: Zn_((s) + Ag_2 O_((s)) to ZnO_((s)) + 2Ag_((s)) , DeltaG^(0)f (Ag_2O) = -11 . 21 kJ mol^(-1) `
` DeltaG^(0)F (ZnO) = -318 . 3 kJ mol^(-1)` Hence ` E_("cell")^(0)` of the button cell is :

A

`3.182 V `

B

`1.71 V `

C

`-1.591V `

D

`1.591V `

Text Solution

Verified by Experts

The correct Answer is:
D
`DeltaG^(0) = DeltaG_f "(products)" - DeltaG_f " (reactant)" = -318 .3 - (11.21) = -3.07 xx 10^(3)` in KJ ........... (1)
`DeltaG^(0) = -nF E^(0)` ......... (2) `:. -nfE^(0) = -307 xx 10^(3)`
` 2 xx 96500 xx E^(0) = 307 xx 10^(3) , E^(0) = (3.07 xx 10^(3))/(2 xx 96500) = + 1.59V`
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