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 intensive property.

4. Absolute electrode potential is 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. Metal reactivity increases.

2. Metal reactivity decreases.

3. No effect on metal.

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.