If at `25^@C`, the standard emf of the cell `|Zn(s)| Zn^2+ (1M) || Cu^2(0.1 M) | Cu (s)` is 1.3 volt, calculate the emf of the cell.

The standard emf of the cell reaction 2 Cu^+ (aq) rarr Cu(s) + Cu^(+2) (aq) is 0.36 volt at 298 k .The equilibrium constant for the reaction is :

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

Calculate the standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

For the cell Zn|Zn^(2+)||Cu^(2+)|Cu if the concentration of Zn^(2+) and Cu^(2+) ions is doubled, the emf of the cell:

What are Electrochemical cells ? What would happen if no salt bridge were used in electrochemical cell like Zn - Cu cell ? Write the Nernst equation to calculate the emf of this cell.

Write the Nernst equation and emf of the following cell at 298 K. (i) Mg(s) |Mg^(2+) ( 0.001 M) || Cu^(2+) ( 0.0001M ) | Cu(s) (ii) Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M) | H_(2)(g) (1 "bar") | Pt(s) Given that, E_(Mg^(2+) //Mg)^(@) = - 2.36V , E_(Cu^(2+) Cu)^(@) = 0.34V, E_(Fe^(2+)Fe)^(@) = -0.44V