Define standard emf of a cell.

The relationship between equilibrium constant and standard emf of a cell is

Calculate the standard emf of the cell having the standard free energy change of the cell reaction is -64.84 kJ for 2 electrons transfer.

The standard electrode potential of Zn^(2+)|ZnandCu^(2+)|Cu are - 0.76 and 0.34 V respectively . The standard e.m.f. of the cell is :

The standard free energy change of the reaction M_((aq))^(+)+e rarrr M_((s)) is -23.125kJ . Calculate the standard emf of the half cell.

The emf of the half cell Cu_((aq))^(2+)//Cu_((s)) containing "0.01 M Cu"^(2+) solution is +0.301 V . Calculate the standard emf of the half cell.

The standard e.m.f. of the cell Zn+Cu^(2+)rarr Cu+Zn^(2+) is 1.10 V at 25^(@)C . The e.m.f. of the cell when 0.1 M Cu^(2+) and 0.1 M Zn^(2+) solutions are used will be

For the cell reaction, Zn(s)+Mg^(2+)(0.1M) hArr Zn^(2+)(1M)+Mg the e.m.f. has been found to be 0.2312 V. The standard e.m.f. of the cell is :

The standard emf of galvanic cell involving 3 moles of electrons in its redos reaction is 0.59V. The equilibrium constant for the reaction of the cell is