Select the correct cell reaction of the cell Ag(s)|Ag^+(aq)"||"Cu^(2+)(aq)"|"Cu(s) :
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 each half cell reaction of the following electrochemical cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)
In the reaction 2Al(s)+6HCl(aq)to6Cl^(-)(aq)+3H_2
Which of the following will increase the voltage of the cell Sn(s)+2Ag^(+)(aq)rarrSn^(2+)(aq)+2Ag(s)
calculate the e.m.f (in V) of the cell: Pt|H_2(g)|BOH(Aq)"||"HA(Aq)|H_2(g)|Pt , 0.1bar 1M 0.1M 1bar Given : K_a(HA)=10^(-7), K_b(BOH)=10^(-6)
Electrode potential of the half Pt(s)|Hg(l)| Hg_(2)Cl_(2)(s) | Cl^(-)(aq) can be incresed by :
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