At what `pH`,given half cell `MnO_(4)^(-)(0.1M)|Mn^(2+)(0.001M)` will have electrode potential of `1.282` _____________`V`? (Nearest Integer)
Given `E_((MnO_(4))^@//Mn^(2+))=1.54V,(2.303RT)/(F)=0.059V`

For the cell Cu (s) | Cu ^(2+) (aq) (0.1 M) || Ag ^(+) (aq) (0.01 M) | Ag (s) the cell potential E _(1) = 0.3095 V For the cell Cu (s) | Cu ^(+2) (aq) (0.01 M) || Ag ^(+) (aq)( 0. 001 M) | Ag (s) the cell potential = _______ xx 10 ^(-2) V. (Round off the Nearest Integer). [Use : (2.303 RT)/(F) =0.059 ]

mf of the following cell at 298 K in V is x""xx10^(-2).Zn|Zn^(2+)(0.1M)||Ag^(+)(0.01M)|Ag The value of x is ______ Rounded off the the nearest integer) Givne E_(Zn^(+)//Zn)^(0)=-0.76V,E_(Ag^(+)//Ag)^(0)=+0.80V,(2.303RT)/(F)=0.059 ]

Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

The magnitude of the change in oxidising power of the MnO_4^(-)//Mn^(2+) couple is x xx 10^(-4)V , if the H^(+) concentration is decreased from 1M to 10^(-4) M at 25^(@)C . (Assume concentration of MnO_4^(-) and Mn^(2+) to be same on change in H^(+) concentration ) . The value of x is ___________. (Rounded off to the nearest integer ) [Given : (2.303 RT)/(F) = 0.059 ]

If DeltaG^(@) for the half cell MnO_(4)^(-) | MnO_(2) in an acid solution is xF then find the value of x. (Given: E_(MnO_(4)^(-) | Mn^(2+))^(@) = 0.34 V, E_(Sn^(4+)|Sn^(2+))^(@) = 0.15 V )

Find the EMF of cell (in volts) formed by connected two half cells: Pt(s) | MnO_(4)^(-) (0.1 M), MnCl_(2) (0.2M) HCl (1 M) Pt(s) | Cr_(2)O_(7)^(2-)(0.1M) CrCl_(3) (0.2M) HCl (0.7 M) [Given E_(MnO_(4)^(-)|Mn^(2+))^(@) =1.51 V, E_(Cr_(2)O_(7)^(2-)| Cr^(3+) = 1.33 V] Give your answer by multiplying with 10.

If /_\G^(@) for the half cell MnO_4^(-)"|"MnO_2 in an acid solution is -xF then find the value of x.(Given: E_(MnO_4^(-)"|"Mn^(2+))^(@)=1.5V,E_(MnO_2"|"Mn^(2+))^(@)=1.25V )