In the electrochemical cell: 
\(\mathrm{Z n   \left|\right. Z n S O_{4}   \left(\right. 0 . 01   M \left.\right)   \left|\right. \left|\right.   C u S O_{4} \left(\right. 1 . 0   M \left.\right)   \left|\right.   C u}, \)$$
the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ is changed to 0.01 M, the emf changes to E₂. From the following, which one is the relationship between E₁ and E₂ ? 
(Given, \(\frac{RT}{F}\) = 0.059)

1. \(\mathrm{E_{1} < E_{2}}\)

2. \(\mathrm{E_{1} > E_{2}}\)

3. \(\mathrm{E_{2} = 0 \neq E_{1}}\)

4. \(\mathrm{E_{1} = E_{2}}\)

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. $∆{\mathrm{G}}^{\mathrm{o}}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>0;<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}<<mspace\; width="1em"></mspace>1$

2. $∆{\mathrm{G}}^{\mathrm{o}}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>0;<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}><mspace\; width="1em"></mspace>1$

3. $∆{\mathrm{G}}^{\mathrm{o}}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>0;<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}><mspace\; width="1em"></mspace>1$

4. $∆{\mathrm{G}}^{\mathrm{o}}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>0;<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}<<mspace\; width="1em"></mspace>1$

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 × 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: