In a half-cell containing `[Tl^(3+)] = 0.1M` and `[Tl^(+)] = 0.01`M, the cell potential is `-1.2496 V` for the reaction `Tl^(+) rightarrow Tl^(3+) + 2e^(-)`. The standard reduction potential of the `Tl^(+3)|Tl^(+1)` couple at `25^(@)`C is:

The potential of the cell for the reaction, M(s)+2H^(+) (1M)rightarrow H_(2) (g) (1atm)+M^(2+) (0.1m) ' is 1.500 V. The standard reduction potential for M^(2+) / M(s) couple is :

The potential of the cell for the reaction, M(s)+2H^(+) (1M)rightarrow H_(2) (g) (1atm)+M^(2+) (0.1m) ' is 1.500 V. The standard reduction potential for M^(2+) / M(s) couple is :

The potential of the following cell is 0.34 V at 25^(@)C calculate the standard reduction potential of the copper half cell Pt|H_(2)(1 atm)| H^(+)(1 M)||Cu^(2+)(1 M)|Cu

The potential of the following cell is 0.34 V at 25^(@)V . Calculate the standard reduction potential of the copper half-cell . Pt| H_(2) ( 1 atm) | H^(+) ( 1M) || Cu^(2+) ( 1M) | Cu

Which is more stable among Tl^(+3) and Tl^(+1) . Why?

The potential of the following cell is 0.34 volt at 25^@ C. Calculate the standard reduction potential of the Copper half cell. Pt //H_(2 (1 atm )) //H_((1M))^(+) // // Cu_((1m))^(2+) // Cu

An electrochemical cell constructed for the reaction : Cu^(2+)(aq) + M(s) rightarrow Cu(s) + M^(2+) (aq) has an E^(@) = 0.75V . The standard reduction potential for Cu^(2+)(aq) is 0.34V. What is the standard reduction potential for M^(2+) (aq)?