Give the Nernst equation of the cell: Ni(s)|NI^(2+)(aq)(0.1M)||Ag^(+)(aq)(0.1M)|Ag(s) and also find the cell potential. given that E^@(Ag^+|Ag)=0.80V, E^@(Ni^(2+)|Ni)=-0.25V
A cell is set up between copper and silver as follows : Cu(s)|Cu^(2+)(aq)||Ag^(+)(aq)|Ag(s) If two half cells work under standard conditions, calculate the emf of the cell. Given E_(Cu^(2+)|Cu)^(@)=0.34V,E_(Ag^(+)//Ag)^(@)=0.80V
The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is
Mg(s)+2Ag^(+)(1M)rarrMg^(+2)(1M)+2Ag(s) Write cell representation for above reaction.
The e.m.f of the cell Cu|Cu^(2+)(aq)||Ag^(+)(aq)|Ag is 0.46V. The e.m.f for the following cell reaciton: 3Cu+6Ag^+ (aq)rarr3Cu^(2+)+6Ag is 0.46y V. The value of y is
The cell Pt|H_(2)(g) (1bar) |H^(+)(aq),pH=x||Cl^(-)(1M)|Hg_(2)Cl_(2)|Hg|Pt has emf of 0.5755 V at 25^(@)C the SOP of calomel electrode is -0.28V then pH of the solution will be
Silver ions are added to a solution with [Br^(-)]=[Cl^(-)]=[CO_(3)^(2-)]=[AsO_(4)^(3-)] =0.1M. Which compound will precipitate with lowest [Ag^(+)] ?
Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: Which of the electrode is negatively charged?
Dopping of AgCl crystals with CdCl_(2) results in:
Consider a cell given below Cu|Cu^(2+)||Cl^-|Cl_2,Pt Write the reactions that occur at anode and cathode.
