Mg(s) + 2Ag⁺(0.0001M) → Mg²⁺(0.130M) + 2Ag(s)

If  E^Ɵ(cell) for the above mentioned cell is 3.17 V, then E(cell) value will be-

(log 13=1.1)

1. 2.87 V
2. 3.08 V
3. 2.96 V
4. 2.68 V

The equilibrium constant value for the given reaction is:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

(Given: E^Ɵ(cell) = 0.46 V)

1. 3.92 × 10¹⁴
2. 3.92 × 10¹⁵
3. 3.92 × 10¹⁶
4. 3.92 × 10¹⁷

The standard electrode potential for Daniell cell is 1.1V. The standard Gibbs energy for the given reaction is-

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

(Given: F = 96487 C mol^–1)

1. 312.27 kJ mol^–1
2. 212.27 kJ mol^–1
3. – 312.27 kJ mol^–1
4. – 212.27 kJ mol^–1

Resistance of a conductivity cell filled with 0.1 mol L^–1 KCl solution is 100 Ω. If the resistance of the same cell when filled with 0.02 mol L^–1 KCl solution is 520 Ω. The conductivity of 0.1 mol L^–1 KCl solution is 1.29 S/m. The molar conductivity of 0.02 mol L^–1 KCl solution is-

1. 134 S cm² mol^–1
2. 124 S cm² mol^–1
3. 144 S cm² mol^–1
4. 154 S cm² mol^–1

The electrical resistance of a column of 0.05 mol L^–1 NaOH solution of diameter 1 cm and length 50 cm is 5.55 × 10³ ohm.

The molar conductivity of the NaOH solution is-

1. 235.4 S cm² mol^–1
2. 229.6 S cm² mol^–1
3. 217.8 S cm² mol^–1
4. 232.2 S cm² mol^–1

Consider the following data:
Λ^°_m(Ca²⁺) = 119.0 S cm²mol^–1 
Λ^°_m(Cl^-) = 76.3 S cm²mol^–1
Λ^°_m(Mg²⁺) = 106.0 S cm²mol^–1
Λ^°_m(\(SO_{4}^{2-}\)) = 160.0 S cm²mol^–1 
 
The correct statement among the following is-

Λ^°_m for NaCl, HCl and NaAc are 126.4, 425.9 and 91.0 S cm²­­­­ mol^–1 respectively. The value of Λ^°_m for HAc is-

The conductivity of 0.001028 mol L^–1 acetic acid is 4.95 ×10^–5 S cm^–1.  if Λ^°_m for acetic acid is 390.5 S cm^2­­­­ mol^–1, Its dissociation constant value is-

1. 1.58 × 10^–5 mol L^–1
2. 1.78 × 10^–5 mol L^–1
3. 1.98 × 10^–5 mol L^–1
4. 2.18 × 10^–5 mol L^–1

What is the mass of copper deposited at the cathode after electrolyzing a solution of CuSO₄ for 10 minutes with a current of 1.5 amperes?

1. 0.36 g
2. 0.48 g
3. 0.30 g
4. 0. 22 g