The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called:
1. Cell potential.
2. Cell emf.
3. Potential difference.
4. Cell voltage.

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

An electrochemical cell can behave like an electrolytic cell when -

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