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?

Find the emf of the cell in which the following reaction takes place at 298 K

Ni(s) + 2Ag⁺ (0.001 M) $$\to$$ Ni²⁺ (0.001 M) + 2Ag(s)

(Given that E$$_{cell}^o$$ = 10.5 V, $${{2.303\,RT} \over F} = 0.059$$ at 298 K)