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Calculate the standard EMF of a cell which invovles the following cell reaction Zn+2Ag^(+)toZn^(2+)+2Ag Given that E_(Zn,Zn^(2+))^(@)=0.76 "volt" and E_(Ag,Ag^(+))^(@)=0.080 volt. |
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Answer» Solution :The cell reaction may be split into two HALF reactioin as: `ZntoZn^(2+)+2e^(-)`(oxidation half reaction) `2Ag^(+)+2e^(-)to2Ag`(Reduction half reaction) Here, we are given STANDARD oxidation potentials as `E_(Zn,Zn^(2+))^(@)=0.76` VOLT and `E_(Ag,Ag^(+))^(@)=0.80` volt We need oxidation potential of zinc electrode but reduction potential of SILVER electrode. Reduction potential of Ag electrode=-Oxidation potentil of Ag electrode =-(-0.80 volt)=+0.80 volt Std. EMF of the cell=Std. oxid. potential of zinc electrode+Std. redn. potential of Ag electrode =+0.76+0.80 volt=1.56 VOLTS. |
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