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.

The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. The cell constant if conductivity of 0.001 M KCl solution at 298 K is 0.146 ×10^-3  S cm^-1 will be: 

1. 0.32 cm^-1

2. 0.47 cm

3. 0.22 cm^-1

4. 0.23 cm

The conductivity of 0.00241 M acetic acid is 7.896 × 10^–5 S cm^–1. If ${\mathrm{\Lambda }}_{\mathrm{m}}^0$ for acetic acid is 390.5 S cm² mol^–1, the dissociation constant will be 
1. \(2.45 \times 10^{-5} \mathrm{~mol} \ \mathrm{~L}^{-1} \)
2. \(1.86 \times 10^{-5} \mathrm{~mol} \ \mathrm{L^{-1}} \)
3. \(3.72 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}} \)
4. \(2.12 \times 10^{-5}\mathrm{~mol} \mathrm{~L^{-1}}\)

A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of nickel(Ni) is deposited at the cathode?
(Given Molar Mass of Ni = 58.7g)

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.