If standard emf `(E^(@))` of a half -cell `Y^(2+)//Y^(+)` is 0.15 V, the standard emf of the half cell `Y^(+)//Y` will be ? Given that the standard emf of cell of full cell is 0.34V.

Define standard emf of a cell.

Define standard emf of a cell.

Define standard emf of a cell.

The magnitude ( but not the sign ) of the standard reduction potentials of two metals X and Y are : Y^(2)+2e^(-) rarr Y |E_(1)^(c-)|=0.34V X^(2)+2e^(-) rarr X |E_(2)^(c-)|=0.25V When the two half cells of X and Y are connected to construct a cell, electrons flow from X to Y . When X is connected to a standard hydrogen electrode (SHE) ,electrons flow from X to SHE . If standard emf (E^(c-)) of a half cell Y^(2)|Y^(o+) is 0.15V , the standard emf of the half cell Y^(o+)|Y will be (a) 0.19V (b) 0.53V (c) 0.49V (d) 0.64V

Standard E^@ of the half cell Fe/ Fe^(2+) is +0.44V and standard E^@ of half cell Cu / Cu^(2+) is -0.32V then:

Standard E^0 of the half cell Fe | Fe^(2+) is +0.44V and standard E^0 of half cell Cu|Cu^(2+) is -0.32V ,then