The standard reduction potential of the `Ag^(o+)|Ag` electrode at `298K` is `0.799V`. Given that for `AgI,K_(sp)=8.7xx10^(-17)`, evaluate the potential of the `Ag^(o+)|Ag` electrode in a saturated solution of `AgI`.

The reduction potential of a hydrogen electrode at pH 10 at 298K is : (p =1 atm)

The standard reduction potential at 298 K for single electrodes are given below.l From this we can tell that

The standard half-cell reduction potential for Ag+|Ag is 0.7991 V at 25^(@)C . Given the experimental value K_(sp) =1.56xx10^(-10) for AgCl, calculate the standard half-cell reduction potential for the AglAgCI electrode.

The standard reduction potential of Cu^(2+)|Cu and Ag^(o+)|Ag electrodes are 0.337 and 0.799V , respectively. Construct a galvanic cell using these electrodes so that its standard EMF is positive. For what concentration of Ag^(o+) will the EMF of the cell , at 25^(@)C , be zero if the concentration of Cu^(2+) is 0.01M ?

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Given the standard reduction potentials. E_(K^(+)//K)^(@)=-2.93V, E_(Ag^(+)//Ag)^(@)=+0.80V, E_(Hg^(+)//Hg)^(@)=0.79V E_(Mg^(+)//Mg)^(@)=-2.37V, E_(Cr^(3+)//Cr)^(@)=-0.74V The correct increasing order of reducing power is:

The standard reduction potentials of Cu^(2+)|Cu and Cu^(2+)|Cu^(o+) are 0.337V and 0.153V , respectively. The standard electrode potential fo Cu^(o+)|Cu half cell in Volts is

The standard reduction potentials of Cu^(2+)|Cu and Cu^(2+)|Cu^(o+) are 0.337V and 0.153V , respectively. The standard electrode potential fo Cu^(o+)|Cu half cell is

The solubiltiy product of silver iodide is 8.3 xx 10^(-17) and the standard potential (reduction) of Ag,Ag^(+) electrode is +0.800 volts at 25^(@)C . The standard potential of Ag,AgI//I^(-) electrode (reduction) from these data is

Calculate the reduction potential for the following half cell reaction at 298 K. Ag^(+)(aq)+e^(-)toAg(s) "Given that" [Ag^(+)]=0.1 M and E^(@)=+0.80 V

Consider the following cell reaction at 298 K : 2Ag^(+)+Cdrarr2Ag+Cd^(2+) The standard reduction potentials (E^(@)) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40V respectively : (1) Write the cell representation. (2) What will be the emf of the cell if the concentration of Cd^(2+) is 0.1 M and that of Ag^(+) is 0.2 M? (3) Will the cell work spontaneously for the condition given in (2) above?