Two half cell reactions are given below.

$$C{o^{3 + }} + {e^ - } \to C{o^{2 + }},\,\,\,\,\,\,\,\,\,E_{C{o^{2 + }}/C{o^{3 + }}}^0 = - 1.81\,V$$

$$2A{l^{3 + }} + 6{e^ - } \to 2Al(s),\,\,\,E_{Al/A{l^{3 + }}}^0 = + 1.66\,V$$

The standard EMF of a cell with feasible redox reaction will be :

Standard electrode potential for the cell with cell reaction

Zn(s) + Cu²⁺(aq) $$\to$$ Zn²⁺(aq) + Cu(s)

is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction. (Given F = 96487 C mol^$$-$$1)

At 298 K, the standard electrode potentials of Cu²⁺ / Cu, Zn²⁺ / Zn, Fe²⁺ / Fe and Ag⁺ / Ag are 0.34 V, $$-$$0.76 V, $$-$$0.44 V V and 0.80 V, respectively.

On the basis of standard electrode potential, predict which of the following reaction cannot occur?

Given below are half cell reactions:

$$MnO_4^ - + 8{H^ + } + 5{e^ - } \to M{n^{2 + }} + 4{H_2}O$$,

$$E_{M{n^{2 + }}/MnO_4^ - }^o = - 1.510\,V$$

$${1 \over 2}{O_2} + 2{H^ + } + 2{e^ - } \to {H_2}O$$

$$E_{{O_2}/{H_2}O}^o = + 1.223\,V$$

Will the permanganate ion, $$MnO_4^ - $$ liberate O₂ from water in the presence of an acid?