Using the Gibbs energy change, ΔG⁰ = +63.3 KJ for the following reaction,
Ag₂CO₃ (s) r2Ag⁺ (aq) + CO₃^2- (aq)
the Ksp of Ag₂CO₃ (s) in water at 25⁰ C is (R= 8.314 JK^-1 mol^-1)

• 3.2 x 10^-26

• 8.0 x 10^-12

• 2.9 x 10^-3

• 2.9 x 10^-3

At 25⁰ molar conductance of 0.1 molar aqueous solutions of ammonium hydroxide is 9.54 ohm^-1 cm² mol^-1 and at infinite dilution, its molar conductance is 238 ohm^-1 cm² mol^-1. The degree of ionisation of ammonium hydroxide at the same concentration and temperature is 

• 2.080%

• 20.800%

• 4.008%

• 4.008%

A button cell used in watches functions as following

The cell potential will be

• 1.10 V

• 0.42 V

• 0.84 V

• 0.84 V

Limiting molar conductivity  of NH₄OH (i.e.,  is equal to 

Standard reduction potentials of the half-reactions are given below.

F₂ (g) +2e^- → 2F^- (aq) ;  E^o = +2.85 V
Cl₂ (g) +2e^- →2Cl^- (aq) ; E^o = +1.36V
Br₂ (l) +2e^- → 2Br^- (aq) ; E^o = +1.06 V
I₂ (s) +2e^- →2I^- (aq); E^o = +0.53 V

The strongest oxidising and reducing agents respectively are

• F₂ and I^-

• Br₂ and Cl^-

• Cl₂ and Br^-

• Cl₂ and Br^-

256.

Molar conductivities (Λ^o_m) at infinite dilution of NaCl, HCl and CH₃COONa are 126.4, 425.9 and 91.0 S Cm² mol^-1 respectively. Λ^o_m for CH₃COOH will be

• 425.5 S cm² mol^-1

• 180.5 S cm² mol^-1

• 290.8 S cm² mol^-1

• 290.8 S cm² mol^-1

The Gibb's energy for the decomposition of Al₂O₃ at 500^o C is as follow
2/3 Al₂O₃ → 4/3 Al + O₂;
Δ_rG = +960 kJ mol^-1
The potential difference needed for the electrolytic reduction aluminium oxide (Al₂O₃) at 500⁰ C is at least 

• 4.5 V

• 3.0 V

• 2.5 V

• 2.5 V

Standard electrode potential of three metal X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be

• Y > X > Z

• Z> X> Y

• X > Y > Z

• X > Y > Z

If the E^o_cell for a given reaction has a negative value then which of the following gives the correct relationships for the values of ΔG^o and K_eq ?

• ΔG^o < 0; K_eq > 1

• ΔG^o < 0; K_eq < 1

• ΔG^o > 0; K_eq < 1

• ΔG^o > 0; K_eq < 1

The electrode potentials for 

Cu²⁺ (aq) + e^- → Cu⁺ (aq) and Cu⁺ (aq) + e^- →Cu (s)

are +0.15 V and +0.50V respectively. The value of  will be 

• 0.325 V 

• 0.650 V

• 0.150 V

• 0.150 V