The correct value of cell potential in volt for the reaction that occurs when the following two half cells are connected, is

$$\begin{aligned} & \mathrm{Fe}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s}), \mathrm{E}^{\circ}=-0.44 \mathrm{~V} \\ & \mathrm{Cr}_2 \mathrm{O}_7^{2-} \text { (aq) }+14 \mathrm{H}^{+}+6 e^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O} \\ & \mathrm{E}^{\circ}=+1.33 \mathrm{~V} \end{aligned}$$

The conductivity of centimolar solution of $$\mathrm{KCl}$$ at $$25^{\circ} \mathrm{C}$$ is $$0.0210 ~\mathrm{ohm}^{-1} \mathrm{~cm}^{-1}$$ and the resistance of the cell containing the solution at $$25^{\circ} \mathrm{C}$$ is $$60 ~\mathrm{ohm}$$. The value of cell constant is -

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 :