Calculate the emf of the cell in which the following reaction takes place: `Ni(s) + 2Ag_((aq))^+ rarr Ni_((aq))^(2+) + 2 Ag (0.002M) (0.160M)` `E_(cell)^@ = 1.05 V`.

Calculate the standard cell potentials of galvanic cell in which the following reactions take place 2Cr_((s)) + 3Cd_((aq))^(2+)rarr 2Cr_(aq)^(3+) + 3Cd E_(Cr)^@ = -0.740 V, E_(Cd)^@ = -0.403 V, Calculate the Delta_rG^@ and equilibrium constant of the reactions.

Formulate a cell for each of the following reactions:- Mg(s) + Br_2(l)rarr Mg^(2+)(aq),+ 2Br^-(aq)

Balance the following equation stepwise. Ag_((s))+HCl_((aq))rarrAgCldarr +H_2uarr

Calculate equilibrium constant for the reaction, Ni_((s)) + 2Ag_((aq))^(2+) rarr Ni_((aq))^(2+) + 2Ag_((s)) at 25^@C E_(Ni)^@ =- 0.25V and E_(Ag)^@ = 0.799V .

Formulate a cell for each of the following reactions:- Sn^(2+)(aq)+2AgCI(s) rarr Sn^(4+)(aq) + 2Ag(s) +2Cl-(aq)

Write shorthand notation for the cell for each of the following reactions :- Cu(aq)^(2+) + 2Ag_(s) + 2Br_(aq)rarrCu_(s)+2AgBr_(s)

Write shorthand notation for the cell for each of the following reactions :- Sn(aq)^(2+) is oxidised by Br_(2(I)

The standard potential of the cell in which the following reaction occurs H_2 (g,1atm) + Cu^(2o+)(1M)rarr2H^(o+)(1M)+Cu(S), ( E^0Cu = 0.34V) is

Consider the following redox reaction Mg_((S)) +Sn_((aq))^(2+) rarr Mg_((aq))^(2+)+Sn_((s)) : Write the cell formula.

Calculate the potential of the following cell at 25^@C . Sn_((s))|Sn^(2+) (0.025M)||Ag^+ (0.015M)|Ag(s) E_(sn)^0 = -0.136V, E_(Ag)^@ = 0.799V .