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1. Consider the given half-cell reactions: 
\(\begin{array}{ll} \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} & \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^0=0.77 \mathrm{~V} \\ 2 \mathrm{I}^{-} \rightarrow \mathrm{I}_2+2 \mathrm{e}^{-} & \mathrm{E}_{\mathrm{I}_2 / \text{I}^-}^{\circ}=0.54 \mathrm{~V} \end{array}\)
The standard electrode potential for the spontaneous reaction in the cell is \(x\times 10^{-2}V~\text{at}~ 298~K.\) 
The value of \(x\) is: (Nearest Integer)
1. 32
2. 23
3. 45
4. 17

2. Given the following reaction:
\(\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\)
E°_cell = 2 V  at 298 K 
The standard Gibbs energy for the given cell reaction in kJ mol^–1 at 298 K is:
(Faraday’s constant, F = 96000 C mol^–1)
1. –384
2. 384
3. 192
4. –192

3. \(\Delta G^o \) for a reversible reaction having equilibrium constant 10^–2 at 27°C will be: 
1. 500R
2. 2.303 × 600R
3. 600R
4. 2.303 × 500R

4. The graph represents the variation of molar conductance (\(\Lambda_m\)) with the square root of concentration (\(\sqrt{C}\)​) for two electrolytes, 'A' and 'B'. Based on the graph, the nature of both electrolytes is:

1. A → Strong Electrolyte, B→ Strong Electrolyte
2. A → Weak Electrolyte, B → Strong Electrolyte
3. A → Strong Electrolyte, B → Weak Electrolyte
4. A → Weak electrolyte, B → Weak Electrolyte

5.

The resistance of a cell containing 0.001 M KCl solution at 298 K is 1500 Ω. The conductivity is 0.146 × 10^–3 S cm^–1. The cell constant would be:

1.	$0.12$ ${\mathrm{cm}}^{-1}$	2.	$0.56$ ${\mathrm{cm}}^{-1}$
3.	$0.22$ ${\mathrm{cm}}^{-1}$	4.	$1.36$ ${\mathrm{cm}}^{-1}$

6.  Match column I with column II and mark the appropriate choice:

	Column I		Column II
(A)	Electrochemical equivalent	(i)	Potential difference \(\times\) Quantity of charge
(B)	Faraday	(ii)	Mass of substance deposited by one coulomb of charge
(C)	Ampere	(iii)	Charge carried by one mole of electrons
(D)	Electrical energy	(iv)	One coulomb of electric charge passed through one second

1. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
2. (A) →(ii), (B)→(iii), (C) →(iv), (D)→ (i)
3. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
4. (A) →(iv), (B)→(i), (C) →(ii), (D)→ (iii)

7. Match the two lists and choose the correct option:

	List-I		List-II
(i)	Ni-Cd cell	(a)	Rechargeable
(ii)	Fuel cell	(b)	Anode \(\left(\mathrm{Zn} \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{e}^{-}\right)\)
(iii)	Mercury cell	(c)	Used in hearing aid
(iv)	Leclanché cell	(d)	Converts combustion energy into electrical energy

1. (i)-(a); (ii)-(d); (iii)-(c), (iv)-(b)
2. (i)-(b); (ii)-(a); (iii)-(c), (iv)-(d)
3. (i)-(d); (ii)-(a); (iii)-(c), (iv)-(b)
4. (i)-(a); (ii)-(b); (iii)-(c), (iv)-(d)

8. The strongest reducing agent on the basis of E° values is: 
1. \(\text A^+ / \text A ;~ E^o = -3.04 \text V \)
2. \(\text B^+ / \text B ;~ E^o = -2.71 \text V \)
3. \(\text C^+ / \text C ;~ E^o = -2.92 \text V \)
4. \(\text D^+ / \text D ;~ E^o = +0.79 \text V \)

9. Match Column I with Column II and mark the appropriate choice:

	Column I		Column II
(A)	\(Pb_{(s)} + SO^{2-}_{4(aq)} \rightarrow\\ PbSO_{4(s)}+ 2 e^-\)	(i)	Rusting of iron
(B)	\( SO^{2-}_{4(aq)} \rightarrow \\S_2O^{2-}_{8(aq)}+ 2 e^-\)	(ii)	Reaction at the anode in lead storage battery
(C)	\(2H_{2(g)} + 4OH^{-}_{(aq)} \rightarrow \\4 H_2O_{(l)}+ 4e^-\)	(iii)	Electrolysis of concentrated  \(H_2SO_4\)
(D)	\(2Fe_{(s)} + O_{2(g)} + 4H^+_{(aq)} \rightarrow \\2Fe^{2+}_{(aq)}+ 2 H_2O_{(l)}\)	(iv)	Reaction at the anode in fuel cell

1. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
2. (A) →(ii), (B)→(iii), (C) →(iv), (D)→ (i)
3. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
4. (A) →(iv), (B)→(i), (C) →(ii), (D)→ (iii)

10. The reduction potential of the hydrogen electrode when in contact with a solution having pH = 8 is:
(Given : \(\text {P}_{H_2} = 1~\text {atm} \))
1. –0.71 V 
2. –0.47 V 
3. –0.95 V 
4. –0.36 V