Mg(s) + 2Ag+(0.0001M) → Mg2+(0.130M) + 2Ag(s)
If EƟ(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: EƟ(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-
1. | For CaCl2 Λ°m is 271.6 S cm2 mol–1 and for MgSO4 Λ°m is 266 S cm2 mol–1. |
2. | For CaCl2 Λ°m is 195.3 S cm2 mol–1 and for MgSO4 Λ°m is 266 S cm2 mol–1. |
3. | For CaCl2 Λ°m is 271.6 S cm2 mol–1 and for MgSO4 Λ°m is 133 S cm2 mol–1. |
4. | For CaCl2 Λ°m is 135.8 S cm2 mol–1 and for MgSO4 Λ°m is 133 S cm2 mol–1. |
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-
1. | 380.9 S cm2 mol–1 | 2. | 390.5 S cm2 mol–1 |
3. | 400 S cm2 mol–1 | 4. | 410.6 S cm2 mol–1 |
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 cm2 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