Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R:

Assertion A : In equation $$\mathrm{\Delta_rG=-nFE_{cell}}$$, value of $$\mathrm{\Delta_rG}$$ depends on n.

Reason R : $$\mathrm{E_{cell}}$$ is an intensive property and $$\mathrm{\Delta_rG}$$ is an extensive property.

In the light of the above statements, choose the correct answer from the options given below:

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?