The cell in which the following reactions occurs:

2Fe³⁺_(aq)+2I^-_(aq)→2Fe²⁺_(aq)+I_2(s) has \(E_{cell}^{o}\)= 0.236 V at 298 K.

The standard Gibbs energy of the cell reaction is -

1.   41.14 kJ mol⁻¹
2.   45.54 kJ mol⁻¹
3. −49.94 kJ mol⁻¹
4. −45.54 kJ mol⁻¹

 

The molar conductivity of 0.025 mol L⁻¹ methanoic acid is 46.1 S cm² mol⁻¹.

The dissociation constant of methanoic acid is-

 Given λ°(H⁺)= 349.6 S cm² mol⁻¹ and λ°(HCOO⁻) = 54.6 S cm² mol

1. \(1.27×10^{-4}mol ~L^{−1}\)
2. \(5.17×10^{-5}mol ~L^{−1}\)
3. \(3.67×10^{-4}mol ~L^{−1}\)
4. \(4.87×10^{-5}mol ~L^{−1}\)

The number of electrons flow through the wire when a current of 0.5 ampere flows through a metallic wire for 2 hours, is-

1. \(6.25×10^{22}\)
2. \(2.25×10^{22}\)
3 \(8.25×10^{22}\)
4. \(4.25×10^{22}\)

The metals among the following that can be  extracted electrolytically is -
1. K
2. Na
3. Al
4. All of the above

 

Rusting of iron is envisaged as setting up of an electrochemical cell because: 

1. Oxidation of iron takes place during rusting.
2. Reduction of iron takes place.
3. Iron shows disproportionation reaction.
4. Oxygen is getting oxidised.

The cell in which the following reactions occurs:

2Fe³⁺_(aq)+2I^-_(aq)→2Fe²⁺_(aq)+I_2(s) has \(E_{cell}^{o}\)= 0.236 V at 298 K.

The standard Gibbs energy of the cell reaction is −45.54 kJ mol⁻¹ . The value of equilibrium constant  of the cell reaction is

1. 10.27 × 10⁹
2. 9.57 × 10⁷
3. 12.17 × 10⁸
4. 7.17 × 10⁶

The emf of the cell in which the following reaction takes place is-

Ni_(s)+2Ag⁺(0.002 M) →Ni²⁺(0.160 M) + 2Ag_(s)
( Given that \(E_{cell}^{o}\)= 1.05 V)

1. E_cell= 9.14 V
2. E_cell= 0.0914 V
3. E_cell= 0.00914 V
4. E_cell= 0.914 V