The reaction from following having top position in EMF series (Std.red. potential) according to their electrode potential at 298 K is: 

1. ${\mathrm{Mg}}^{2+}+2{\mathrm{e}}^{-}\to {\mathrm{Mg}}_{\left(\mathrm{s}\right)}$

2. ${\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}\to {\mathrm{Fe}}_{\left(\mathrm{s}\right)}$

3. ${\mathrm{Au}}^{3+}+3{\mathrm{e}}^{-}\to {\mathrm{Au}}_{\left(\mathrm{s}\right)}$

4. ${\mathrm{K}}^{+}+{\mathrm{le}}^{-}\to {\mathrm{K}}_{\left(\mathrm{s}\right)}$

One liter of 0.5 M KCl solution is electrolyzed for one minute in a current of 1.608 mA. Considering 100 % efficiency, the pH of the resulting solution will be : 

Absolute electrode potential of an electrode can't be measured because:

1. Oxidation or reduction can not occur alone.

2. Oxidation or reduction can occur alone.

3. Absolute electrode potential is an intensive property.

4. Absolute electrode potential is an extensive property.

 E⁰_cell for  feasible type cell reaction is : 

1.E⁰_cell = 0

2. E⁰_cell > 0

3. E⁰_cell < 0

4. None of the above.

E⁰_cell for  non-feasible type cell reaction is :

1. \(E_{cell}^{\circ }\) = Positive
2. \(E_{cell}^{\circ }\)= Negative
3. \(E_{cell}^{\circ }\) = Zero
4. None of the above.

 E_cell =0 or ${∆}_r$G =0  this condition is applicable on : 

1. Spontaneous reaction

2. Equilibrium reaction

3. Non-Equilibrium reaction

4. None of the above

The negative sign in the expression E^o_Zn²⁺/Zn = -0.76 V indicates : 

1. The reactivity of the metal increases.

2. The reactivity of the metal decreases.

3. There is no effect on the metal's reactivity.

4. None of the above.

Electrode potential is the potential difference between the -

1. Electrode and the electrolyte.

2. Anode and Cathode.

3. Anode and Atmosphere.

4. Cathode and Atmosphere.

Molten sodium chloride conducts electricity due to the presence of: 

1. Free ions.

2. Free molecules.

3. Free electrons.

4. Atoms of sodium and chlorine.