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

1. $∆{\mathrm{G}}^{\mathrm{o}} > 0; {\mathrm{K}}_{\mathrm{eq}}< 1$

2. $∆{\mathrm{G}}^{\mathrm{o}} > 0; {\mathrm{K}}_{\mathrm{eq}}> 1$

3. $∆{\mathrm{G}}^{\mathrm{o}} < 0; {\mathrm{K}}_{\mathrm{eq}}> 1$

4. $∆{\mathrm{G}}^{\mathrm{o}} < 0; {\mathrm{K}}_{\mathrm{eq}}< 1$

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Charge on electron = 1.60 × 10^–19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$

Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below: 
 
Then the species undergoing disproportionation is:-

The pressure of H₂ required to make the potential of H₂ - electrode zero in pure water at 298 K is:

A device that converts the energy of combustion of fuels, like hydrogen and methane, directly into electrical energy is known as: 

When 0.1 mol MnO₄^2- is oxidized the quantity of electricity required to completely oxidise MnO₄^2--  to MnO₄^- is: 

1. 96500 C

2. 2 x 96500 C

3. 9650 C

4. 96.50 C

The weight of silver (at.wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of O₂ at STP will be:

1. 5.4 g

2. 10.8 g

3. 54.0 g

4. 108.0 g

A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 10 and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of the electrode would be: 

If half-cell potentials are-

The cell potential will be: