The incorrect statement about an inert electrode in a cell is:

1.	It does not participate in the cell reaction.
2.	It provides a surface either for oxidation or for the reduction reaction.
3.	It provides a surface for the conduction of electrons.
4.	It provides a surface for redox reaction.

An electrochemical cell behaves as an electrolytic cell when the externally applied potential (Eext)
becomes greater than the cell potential (Ecell). Which of the following conditions is correct?

1. E_cell = 0

2. E_cell > E_ext

3. E_ext > E_cell

4. E_cell = E_ext

The incorrect statement about the solution of electrolytes is:

Using the data given below find out the strongest reducing agent.

$\begin{array}{l}{E}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}^{⊝}=1.33\mathrm{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>;<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>E_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}^{\ominus }=1.36\mathrm{V}\\ E_{\mathrm{Mn}{0}_4^{-}/{\mathrm{Mn}}^{2+}}^{⊝}=1.51\mathrm{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>;\hspace{0.17em}{E}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{\ominus }=-0.74\mathrm{V}\end{array}$

1.  Cl^-

2.  Cr

3.  Cr³⁺

4.  Mn²⁺

Using the data given below find out the strongest oxidizing agent.

\(\mathrm{E_{Cr_{2} O_{7}^{2 -} / Cr^{3 +}}^{\ominus} = 1 . 33 V     ;     E_{Cl_{2} / Cl^{-}}^{\ominus} = 1 . 36 V \\ E_{Mn O_{4}^{-} / Mn^{2 +}}^{\ominus} = 1 . 51 V         ;    E_{Cr^{3 +} / Cr}^{\ominus} = - 0 . 74 V}\)

$\begin{array}{l}{E}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}^{⊝}=1.33\mathrm{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>;<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>E_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}^{\ominus }=1.36\mathrm{V}\\ E_{\mathrm{Mn}{\mathrm{O}}_4^{-}/{\mathrm{Mn}}^{2+}}^{⊝}=1.51\mathrm{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>;\hspace{0.17em}{E}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{\ominus }=-0.74\mathrm{V}\end{array}$

Based on the given data, identify the option that correctly lists the order of reducing power.

1.  Cr³⁺ < Cl^– < Mn²⁺ < Cr

2.  Mn²⁺ < Cl^– < Cr³⁺ < Cr

3.  Cr³⁺ < Cl^– < Cr₂O₇^2– < MnO₄^–

4.  Mn²⁺ < Cr³⁺ < Cl^– < Cr

$\begin{array}{l}{E}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}^{⊝}=1.33\mathrm{V};<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>E_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}^{\ominus }=1.36\mathrm{V}\\ E_{\mathrm{Mn}{\mathrm{O}}_4^{-}/{\mathrm{Mn}}^{2+}}^{⊝}=1.51\mathrm{V};\hspace{0.17em}{E}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{\ominus }=-0.74\mathrm{V}\end{array}$

Use the data given above to find out the most stable ion in its reduced form.

The most stable oxidized species among the following is: 
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)

The quantity of charge required to obtain one mole of aluminium from Al₂O₃ is :

1.  1 F

2.  6 F

3.  3 F

4.  2 F

The cell constant of a conductivity cell-