Select the correct cell reaction of the cell Pt(s)|Cl_2(g)|Cl^(-)(aq)"||"Ag^+(aq)|Ag(s) :
Calculate the standard Gibbs energy for the cell : Zn(s)+Zn^(2+)(aq)||Cu^(2+)(aq)|Cu(s) E_((Zn^(2+)//Zn)^(@))=-0.76V,E_((Cu^(2+)//Cu))^(@)=0.34V , F=96500 C .
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
Based on the cell notation for a spontaneous reaction, at the anode: Ag(s)"|"AgCl(s)"|"Cl^(-)(aq)"||"Br^(-)(aq)"|"Br_2(l)"|"C(s)
Write Nernst equation and cell reaction of the following cell: Zn|Zn^(2+)||Cu^(2+)|Cu
Which graph correctly correlates E_(cell) as a function of concentration for the cell Zn(s)+2Ag^+(aq)toZn^(2+)(aq)+2Ag(s), E_(cell)^(@)=1.56V y-axis: E_(cell) , X-axis: log_(10)"([Zn^(2+)])/([Ag^+]^2)
Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: The carriers of the current in the cell.
Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: Individual reaction at each electrode.
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?
Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V