1.

At 25^(@)C temperature, if for given unknown half cell has 0.34 Volt potential, then calculate standard reduction potential for copper : Pt|H_(2(g))(1" atm")|H_((1M))^(+)||Cu_((1M))^(2+)|Cu

Answer»

`-0.34` Volt
`-3.4` Volt
`+0.34` Volt
`+3.4` Volt

Solution :Reaction : `underset(1atm)(H_(2(g))+underset(1M)(Cu_((aq))^(2+)) to underset(1M)(2H_((aq))^(+))+Cu_((S))`
Oxidation : `H_(2(g)) to 2H_((aq))^(+)+2e^(-) , E_(RED)^(@)=`zero
REDUCTION : `Cu_((aq))^(2+)+2e^(-) to Cu_((S)),""E_(red)^(@)=(?)`
`E_(cell)^(@)=E_(red)^(@)("CATHODE")-E_(red)^(@)("ANODE")`
`therefore 0.34=E_(Cu^(2+)//Cu)^(@)-E_(H^(+)//H_(2))^(@)`
`therefore 0.34V=E_(Cu^(2+)//Cu)^(@)-0.0`
`therefore E_(Cu^(2+)//Cu)^(@)=+0.34V`.


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