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 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 standard reduction potential of Cu^(2+)//Cu and Cu^(2+)//Cu^(+) are 0.337 and 0.153 respectively. The standard electrode potential of Cu^(+)//Cu half - cell is

The standard reduction potential of Pb and Zn electrodes are -0.12 6 and -0.763 volts respectively . The e.m.f of the cell Zn|Zn^(2+)(0.1M)||Pb^(2+)(1M)|Pb is

The standard reduction potential for silver electrode is +0.80 V. It is connected to a standard hydrogen electrode to make a galvanic cell. State whether silver electrode will act as anode or cathode.

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 .

If the standard electrode poten tial of Cu^(2+)//Cu electrode is 0.34V. What is the electrode potential of 0.01 M concentration of Cu^(2+) ?

Consider the reaction 2Ag^(+) +Cd to 2Ag to 2Ag +Cd^(2+) . The standard reduction potentials of Ag^(+)//Ag and Cd^(2+)//Cd are + 0.80 volt and - 0.40, respectively. (i) Give the cell representation. (ii) What is the standard cell emf. E^(Theta) ? (iii) What will the emf of the cell if concentration of Cd^(2+) is 0.1 M and Ag^(+) is 0.2 M? (iv) Will the cell work spontaneously for the condition given in (ii) above ?

A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of 10^(-6)M hydrogen ions. The EMF of the cell is 0.118V at 25^(@)C . Calculate the concentration of hydrogen ions at the positive electrode.

The standard electrode potential a Ag^(+)//Ag is +0.80 V and of Cu^(2+)//Cu is +0.34 V. These electrodes are connected through a salt bridge and if :