State the factors that influence the value of cell potential of the following cell: `Mg(s)|Mg^+2(aq)||Ag^+(aq)|Ag(s)`

Write the Nernst equation to calculate the cell potential of Mg (s) | Mg^(2+) (aq) || Ag^(+) |Ag .

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

Derive the Nernst equation for the electrode potential of the electrode M^(n+) (aq) + n e^- rarr M(s)

Which will increase the voltage of the cell Sn(s) +2Ag^+(aq)rarr Sn^(2+)(aq)+2Ag(s) :

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 .

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 each half cell reaction and also the net cell reaction for a cell. (i) Cu[Cu^(+ +(aq))][Ag^(+(aq))]Ag (ii) Cd[Cd^(+2)][Ni^(+2)]Ni