Cu⁺(aq) is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction 

2Cu⁺(aq) $\rightleftharpoons$Cu²⁺(aq) + Cu(s)

Choose the correct E0 for above reaction if E⁰_cu²⁺/cu = 0.34 V and E⁰_cu²⁺/cu+ = 0.15 V 

1. -0.38 V

2. +4.9 V

3. +0.38 V

4. -0.19 V

For the reductidon of silver ions with copper metal, the standard  cell potential was found to be + 0.46 V at 25⁰C. The value of standard Gibbs energy($\Delta$G⁰⁾ will be ;
(F = 96500 Cmol^-1)

1. -89.0 KJ

2. -89.0 J

3. -44.5 KJ

4. -98.0 KJ

When NaCl solution is electrolysed using Pt electrodes then pH of solution

1. Increases

2. Decreases

3. Remains same

4. Firstly increases and then decreases

If the E°_cell for a given reaction has a negative value, which of the following gives correct relationships for the values of $∆$G° and K_eq ?

(1) $∆$G° >0;  K_eq< 1

(2) $∆$G° >0; K_eq>1

(3) $∆$G° < 0; K_eq> 1

(4) $∆$G° <0; K_eq< 1

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 for the pentane-oxygen fuel cell is

(1) 1.968 V

(2) 2.0968 V

(3) 1.0968 V

(4) 0.0968 V

The equilibrium constant of the reaction:

Cu (s) + 2Ag⁺ (aq) $\to$Cu²⁺ (aq) + 2Ag(s) ;

E^o = 0.46 V at 298 K is:

The E° in the given diagram is,

(1) 0.5

(2) 0.6

(3) 0.7

(4) 0.8

At 298K the standard free energy of formation of H₂O(l) is –237.20kJ/mole while that of its ionisation into H+ iion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

H₂(g,1 bar) | H⁺ (1M) || OH^–(1M) | O₂ (g, 1bar)

(1) 0.40 V

(2) 0.81 V

(3) 1.23 V

(4) –0.40 V

Which of the following cell can produce more electric work.

(1) pt,H₂|NH₄Cl||0.1MCH₃COOH|H₂,pt

(2) pt,H₂|0.1MHCl||0.1MNaOH|H₂,pt

(3) pt,H₂|0.1MHCl||0.1MCH₃COOK|H₂,pt

(4) pt,H₂|0.1MCH₃COOK||0.1MHCl|H₂,pt

At what $\frac{\left[{\mathrm{Br}}^{\mathrm{-}}\right]}{\sqrt{\left[{\mathrm{CO}}_3^{2-}\right]}}$ does the following cell have its reaction at equilibrium?

Ag(s) | Ag₂CO₃(s) | Na₂CO₃ (aq) || KBr(aq) | AgBr(s) | Ag(s)

K_SP = 8 × 10^–12 for Ag₂CO₃ and K_SP = 4 × 10^–13 for AgBr

(1) $\sqrt{1}$ × 10^–7

(2) $\sqrt{2}$ × 10^–7

(3) $\sqrt{3}$ × 10^–7

(4) $\sqrt{4}$ × 10^–7