The standard emf for the cell reaction `Zn +Cu^(2) rarr Zn^(2+) +Cu` is `1.10` volt at `25^(@)C`. The emf for the cell reaction when `0.1M Cu^(2+)` and `0.1 Zn^(2+)` solutions are used at `25^(@)C` is

The standard emf for the cell cell reaction Zn + Cu^(2+) rarr Zn^(2+) + Cu is 1.10 volt at 25^@ C . The emf for the cell reaction when 0.1 M Cu^(2+) and 0.1 M ZN^(2+) solutions are used at 25^@ =C is .

The cell reaction Zn(s) + Cu^(+2)rarr Zn^(+2) + Cu(s) is best represented as :

The standard emf for the cell reaction, 2Cu^(+)(aq)toCu(s)+Cu^(2+)(aq) is 0.36V at 298K . The equilibrium constant of the reaction is

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

The standard potential of the cell reaction Zn+Cl_(2)rarr Zn^(2+)+2Cl^(-) is 2.10V .Then the emf of the cell Zn|Zn^(+2)(0.05M)|Cl^(-)(0.2M)|Cl_(2),Pt would be

The measured e.m.f. at 25^(@)C for the cell reaction, Zn(s) +XCu^(2+)._((eq))(0.1M) rarr Cu(s) ._((aq)) +Zn^(2+)(1.0M) is 1.3 volt, calculate E^(@) for the cell reaction.

The standard EMF of the cell reaction 1/2Cu(s)+1/2Cl_2(g) to 1/2Cu^(2+)+Cl^- is 0.2 V. The value of /_\G^0 will be

E^(o) for the reaction Fe + Zn^(2+) rarr Zn + Fe^(2+) is – 0.35 V. The given cell reaction is :

E^(@) for the electrochemical cell Zn(s)|Zn^(2+) 1 M (Aq.)||Cu^(2+) 1 M (aq.)|Cu(s) is 1.10 V at 25^(@)C . The equilibrium constant for the cell reaction, Zn(s) +Cu^(2+) (aq.) hArr Zn^(2+) (aq.)+Cu(s) Will be :

Zn(s) + Cu^(2+)(aq) rarr Zn^(2+)(aq) + Cu(s) The cell representation for the above redox reaction is