Given, 
(i) Cu²⁺ + 2e^- → Cu,     E^o = 0.337 V

(ii) Cu²⁺ +e^- → Cu⁺, E^o = 0.153

Electrode potential, E^o for the reaction,
Cu +e^- →Cu, will be 

• 0.52 V

• 0.90 V

• 0.30 V

• 0.30 V

The values of ΔH and ΔSfor the reaction, C_(graphite) + CO₂  → 2 CO (g) are 170 kJ and 170 JK^-1 respectively. This reaction will be spontaneous at 

• 710 K

• 910 K

• 1110 K

• 1110 K

273.

Kohlrausch's law states that at

• finite dilution, each ion makes a definite contribution to the equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.

• infinite dilution, each ion makes a definite contribution to the equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte.

• infinite dilution, each ion makes a definite contribution to the conductance of an electrolyte whatever be the nature of the other ions of the electrolyte.

• infinite dilution, each ion makes a definite contribution to the conductance of an electrolyte whatever be the nature of the other ions of the electrolyte.

Standard free energies of formation (in kJ/mol) at 298 K are -237.2, 394.4 and -8.2 for H₂O (l), CO₂ (g) and pentane (g),  respectively. The value of E_cell^o for pentane-oxygen fuel cell is

• 1.968 V

• 2.0968 V

• 1.0968 V

• 1.0968 V

The equilibrium constant of the reaction:

Cu (s) + 2 Ag⁺ (aq) →  Cu²⁺ (aq) + 2 Ag (s);

E^o = 0.46 V at 298 K

• 2.4 x 10¹⁰

• 2.0 x 10¹⁰

• 4.0 x 10¹⁰

• 4.0 x 10¹⁰

The efficiency of a fuel cell is given by:

If  the standard emf of the reaction:

Fe + 2 Fe³⁺ →3Fe²⁺

will be:

• 0.330 V

• 1.653 V

• 1.212 V
• 1.212 V

A hypothetical electrochemical cell is shown below
A^- | A⁺ (xM)|| B⁺ (yM)|B⁺

The emf measured is +0.20 V. The cell reaction is:

• A⁺ + B  →  A + B⁺

• A⁺ + e^-  →  A ; B⁺ + e^-  → B^-

• the cell reaction cannot be predicted

• the cell reaction cannot be predicted

Concentration of the Ag+ ions in a saturated solution of Ag₂C₂O₄ is 2.2 ×10^–4 mol L^–1. Solubility product

• 2.42 × 10^–8

• 2.66 × 10^–12

• 4.5 × 10^–11

• 4.5 × 10^–11

In the electrochemical cell :
Zn|ZnSO₄(0.01M)||CuSO₄(1.0 M)|Cu, the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ changed to 0.01 M, the emf changes to E₂. From the following, which one is the relationship between E₁ and E₂?
(Given, RT/F= 0.059)

• E₁= E₂

• E₁< E₂

• E₁> E₂

• E₁> E₂