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)

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.

 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

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.

 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.

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.