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The standard electrode potential a Ag^(+...

The standard electrode potential a `Ag^(+)//Ag` is +0.80 V and of `Cu^(2+)//Cu` is +0.34 V. These electrodes are connected through a salt bridge and if :

A

Copper electrode work like cathode, then `E_("cell")^(@)` is `-0.34 V`

B

Silver electrode work like anode then `E_("cell")^(@)` is `+0.46 V`

C

Copper electrode work like anode then `E_("cell")^(@)` is `-0.30 V`

D

Silver electrode work like cathode then `E_("cell")^(@)` is `-0.34 V`

Text Solution

Verified by Experts

The correct Answer is:
C
Cell reaction is-
`Cu(s) + 2Ag^(+) (aq) to Cu^(2+) (aq) + 2Ag(s)`
Two half cell reaction is-
`Cu(s) to Cu^(2+) (aq) + 2e^(-)` oxidation (anode)
`Ag^(+) (aq) + e^(-) to Ag(s)` Reduction (cathode)
`E_("cell") = E_("OX") -E_("red") = 0.80 - 0.34 = + 0.46` V
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