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[ sider a cell composed of two half-cells Cu(s)|Cu^(2+)(aq) and Ag(s)|Ag^(+)(aq). Calculate (a) the standard cell ntial and (b) the cell potential when [Cu^(2+)] is 2M and [Ag^(+)] is 0.05M. A E^(ominus)(Cu^(2+)/Cu)=0.34V[E^(ominus)(Ag^(+)/Ag)=0.80V,R=8.314JK^(-1)mol^(-1).500Cmol^(-1).]]

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Consider a cell composed of two cells: (i). Cu(s)Cu^(2+)(aq) and (ii). Ag(s)|Ag^(+)(aq) (b). The cell potential when [Cu^(2+)]=2M and |Ag^(+)|=0.05M [Given: C_(Cu^(2+)//Cu)^(@)=+0.344V,E_(Ag^(+)//Ag)^(@)=+0.80V]

Consider a cell composed of two cells: (i). Cu(s)Cu^(2+)(aq) and (ii). Ag(s)|Ag^(+)(aq) (b). The cell potential when [Cu^(2+)]=2M and |Ag^(+)|=0.05M [Given: C_(Cu^(2+)//Cu)^(@)=+0.344V,E_(Ag^(+)//Ag)^(@)=+0.80V]

A cell is represented in the following way. Cu(s)|Cu^(2+)(aq) || Ag^+(aq)|Ag(s) Write the half cell reactions.

Calculate the standard reduction potential of (Ag^+)/ (Ag) electrode when the cell potential for the cell Cu | Cu^2+ (1M) | | Ag^+(1M) | Ag is 0.46 V .

The e.m.f. of the cell at 25^(@)C Cu"|"Cu^(2+)(0.01M)"||"Ag^(+)(0.1M)"|"Ag is [E^(@)(Cu^(2+)"|"Cu)=0.34V, E^(@)(Ag^(+)"|"Ag)=0.80V]

The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu [E^@ for Zn^(2+)//Zn=-0.76V, E^@ for Cu^(2+)//Cu=+0.34V]

Calculate the emf of the cell Cu(s) | Cu^(2+) (aq) || Ag^(+)(aq) | Ag(s) Given, E_((Cu^(2+))//(Cu))=+ 0.34 V, E_((Ag^(+))//( Ag)) = 0.80 V

The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is