Derive Nerst equation for EMF of the following cell. `Zn (s) + Cu^2+ (aq) rarr Zn^2+ (aq) + Cu(s)`

Calculate the standard emf of the cell having the cell reaction. Zn(s) + Co^(2+) ( aq) rarr Zn^(2+) ( aq) + Co(s) E_(Zn//Zn^(2+)) ^(@) = 0.76V, E_(Co//Co^(2+))^(@) = 0.25V

What do you mean by an electro chemical cell? Write the cell representation for the cell Zn(s) + CuSO_4(aq) rarr ZnSO_4(aq) + Cu(s) .

What is meant by electrode potential? Explain in the half cell reactions of Zn(s) + Cu^(2+) ( aq) rarr Zn^(2+) (aq) + Cu(s)

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

Formulate the galvanic cell in which the following reaction takes place. Zn (s) + 2Ag^(+) ( aq) rarr Zn^(2+) (aq) + 2Ag(s) (i) Which one of its electrodes is negatively charged ? (ii) The reaction taking place at each of its electrode. (iii) The carriers of current within this cell.

Write the Nernst equation for the electrode reaction: Cu_(aq)^(2+) + 2e rarr Cu(s)

In the button cells, widely used in watches and other devices, the following reaction takes place Zn (s) + Ag_(2) O(s) + H_(2) O (l) rarrZn^(2+) (aq) + 2Ag(s) + 2OH^(-) (aq) Determine E^(@) and Delta G^(@) for the reaction. (Given, E_(Ag^(+)//Ag)^(@) = + 0.80 V, E_(Zn^(2+)//Zn)^(@) = -0.76 V )

Represent the galvanic cell in which the reaction, Zn(s) + Cu^(2+) (aq) rarr Zn^(2+) (aq) + Cu(s) take place.