ElectroChemistry = B5P

1. ${ 1 \over \wedge_M}$ is plotted against $C\times \wedge_M$ for an aq. solution of caproic acid. It results into a straight line having slope = $\alpha _1$ and intercept on Y-axis = $\alpha_2$. Find ${ 1 \over \alpha_1 } \times { 1 \over \alpha_2}$:
[Where : $\wedge_M$= Molar conductivity
$\wedge^\circ _M$ = Limiting molar conductivity
C= molar concentration
$K_a$ = Acid dissociation constant of caproic acid]
Choose the correct option:

1.	$K_a \times (\wedge^\circ _M )^2$	2.	$K_a \times {1 \over (\wedge^\circ _M )^3}$
3.	$K_a \times {1 \over (\wedge^\circ _M )^2}$	4.	$K_a\times (\wedge^\circ _M )^3 $

2. Consider the following standard electrode potentials and calculate the equilibrium constant at $25^{\circ} \mathrm{C}$ for the given disproportionation reaction:
$3 \mathrm{Mn}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Mn}(s)+2 \mathrm{Mn}^{3+}(\mathrm{aq})$
The standard electrode potentials are:$\begin{aligned} & \mathrm{Mn}^{3+}(\mathrm{aq})+e^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq}) ;~~~~ E^{\circ}=1.51 \mathrm{~V} \\ & \mathrm{Mn}^{2+}(\mathrm{aq})+2 e^{-} \rightarrow \mathrm{Mn}(s) ;~~~~~~~ E^{\circ}=-1.185 \mathrm{~V} \end{aligned}$

1.	$1.2 \times 10^{-43}$	2.	$2.4 \times 10^{-73}$
3.	$6.3 \times 10^{-92}$	4.	$1.5 \times 10^{-62}$

3. Given below are two statements :

Statement I	For $\mathrm{Kl},$ molar conductivity increases steeply with dilution.
Statement II	For carbonic acid, molar conductivity increases slowly with dilution.

In the light of the above statements, choose the correct answer from the options given below :

1.	Statement I is incorrect and Statement II is correct.
2.	Both Statement I and Statement II are correct.
3.	Both Statement I and Statement II are incorrect.
4.	Statement I is correct and Statement II is incorrect.

4. Given that:
$\begin{array}{ll} \mathrm{Zn}^{2+}(a q)+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(s) & E_{\text {red }}^{\circ}=-0.76 \mathrm{~V} \\ \mathrm{Cr}^{3+}(a q)+3 \mathrm{e}^{-} \rightarrow \mathrm{Cr}(s) & E_{\text {red }}^{\circ}=-0.74 \mathrm{~V} \end{array}$
Calculate the equilibrium constant K for the following balanced reaction :
$3 \mathrm{Zn}(s)+2 \mathrm{Cr}^{3+}(a q) \rightarrow 3 \mathrm{Zn}^{2+}(a q)+2 \mathrm{Cr}(s)$
1. $K= e^{-0.02}$
2. $K= e^{0.02}$
3. $K= e^{4.7}$
4. $K= e^{8.0}$

5. Given the following notation for an electrochemical cell:
$\mathrm{{Pt}({s})\left|{H}_2({~g})\right| {H}^{+}({aq}) \| {Ag}^{+}({aq}) \mid {Ag}({s})}$
Which of the following represents the overall balanced (net) cell reaction?
1. $\mathrm {H}_2 \text {(g)} + \mathrm {Ag}^+ \text {(aq)}→ 2 \mathrm {H}^+ \text {(aq)} + \mathrm {Ag} \text {(s)}$
2. $\mathrm {H}_2 \text {(g)} + \mathrm {Ag} \text {(s)} →\mathrm{H}^+ \text {(aq)} + \mathrm {Ag^+} \text {(aq)}$
3. $\mathrm {Ag} \text {(s)} + \mathrm {H}^+ \text {(aq)} → \mathrm {Ag}^+ \text {(aq)}+\mathrm {H}_2 \text {(g)}$
4. None of the above

6. Which of the following compounds is incorrectly classified?
1. $\text{NaF}$ is an electrolyte.
2. $\text{CH}_3\text{OH}$ is a weak electrolyte.
3. $ \text{Mg(C}_2\text{H}_3\text{O}_2)$ is an electrolyte.
4. $\text{CH}_3\text{CH}_2\text{COOH}$ is a weak electrolyte.

7. A cell diagram shown below contains one liter of buffer solution of
$\mathrm{H} A\left(\mathrm{p} K_a=4\right)$ and $\mathrm{NaA}$ in both compartments. What is the cell e.m.f?

1.	0.03 V	2.	0.06 V
3.	-0.06 V	4.	-0.03 V

8. A solution containing one mole per litre of each $Cu(NO_3)_2; AgNO_3; Hg_2(NO_3)_2$ is being
electrolysed by using inert electrodes. The values of standard electrode potentials in volts
(reduction potentials) are:
$\begin{aligned} & \mathrm{Ag} / \mathrm{Ag}^{+}=+0.80,2 \mathrm{Hg} / \mathrm{Hg}_2^{++}=+0.79 \\ & \mathrm{Cu} / \mathrm{Cu}^{++}=+0.34, \mathrm{Mg} / \mathrm{Mg}^{++}=-2.37 \end{aligned}$
With increasing voltage, the sequence of deposition of metals on the cathode will be :
1. Ag, Hg, Cu, Mg
2. Mg, Cu, Hg, Ag
3. Ag, Hg, Cu
4. Cu, Hg, Ag

9.

The standard reduction potentials of $\mathrm{Cu}^{2+} \mid \mathrm{Cu} \text { and } \mathrm{Cu}^{2+} \mid \mathrm{Cu}^{+}$ are 0.337 V and 0.153V respectively. The standard electrode potential of Cu⁺|Cu half cell is:
1. 0.184 V
2. 0.827 V
3. 0.521 V
4. 0.490 V

10. In the electrolytic cell, the flow of electrons comes from :

1.	Cathode to the anode in solution.
2.	Cathode to anode through external supply.
3.	Cathode to anode through the internal supply.
4.	Anode to the cathode through the internal supply.

11. Identify the correct statement:

1.	The corrosion of iron can be minimised by forming contact with another metal with a higher reduction potential.
2.	Iron corrodes in oxygen-free water
3.	The corrosion of iron can be minimised by forming an impermeable barrier
4.	Iron corrodes more rapidly in salt water because its electrochemical potential is higher.

12. An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these mixtures is given in List II. Match List I with List II and select the correct answer using the codes given below the table:

	List-I		List-II
(P)		(i)	Conductivity decreases and then increases.
(Q)		(ii)	Conductivity decreases and then does not change much.
(R)		(iii)	Conductivity increases and then does not change much.
(S)		(iv)	Conductivity does not change much and then increases.

Codes:

	P	Q	R	S
1.	(iii)	(iv)	(ii)	(i)
2.	(iv)	(iii)	(ii)	(i)
3.	(ii)	(iii)	(iv)	(i)
4.	(i)	(iv)	(iii)	(ii)

13. When $\mathrm{AgNO}_3$ (aq.) is gradually added to an aqueous KCl solution, and the conductivity of the solution is measured, what does the plot of conductance (Λ) versus the volume of $\mathrm{AgNO}_3$ (aq.) show?

1.		2.
3.		4.

14. Which of the following equations represents the reaction occurring in a nickel-cadmium battery?

1.	$\small{\mathrm{Cd}_{(\mathrm{s})}+\mathrm{NiO}_{2(\mathrm{~s})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{Cd}(\mathrm{OH})_{2(\mathrm{~s})}+\mathrm{Ni}(\mathrm{OH})_{2(\mathrm{~s})}}$
2.	$\small {Cd_{(s)} + NiO_{2{(s)}} + 2OH^-_{(aq)} \rightarrow Ni{(s)} + Cd(OH)_{2{(s)}}}$
3.	$\small {Ni_{(s)}+ Cd(OH)_{2{(s)} }\rightarrow Cd_{(s)}+ Ni(OH)_{2{(s)}}}$
4.	$\small {Ni(OH)_{2(s)}+Cd(OH)_{2(s)} \rightarrow Ni_{(s)} + Cd_{(s)}+2H_2O(l)}$

15. Which among the following represents a concentration cell?

1.	$I^-(aq) \|I_2(s) \|\| Br_2(l) \|Br^-(aq) $
2.	$Zn(s) \| Zn^{2+} (aq) \|\| Pb^{2+} (aq) \| Pb(s) $
3.	$Pt,H_2(g) \|H_2O(l) \| OH^-(aq) \|\|O_2(g) \|OH^- (aq), Pt$
4.	$Ag(s) \| Ag^+ (aq) \|\| Ag^+ (aq) \|Ag(s) $

16. Which of the following statements about the lead storage battery is incorrect?

(A)	During charging, PbSO₄ on the anode is converted into PbO₂.
(B)	During charging, PbSO₄ on the cathode is converted into PbO₂.
(C)	The lead storage battery consists of a grid of lead packed with PbO₂ as the anode.
(D)	The lead storage battery uses a ~38% solution of sulfuric acid as an electrolyte.

1. (B) and (D) only
2. (B), (C) and (D) only
3. (A), (B) and (D) only
4. (B) and (C) only

17. The molar conductance of a solution, given its conductivity (0.248 S m^-1) and concentration (0.2 mol m^-3) is:
1. 0.124 S cm² mol^-1
2. 1.24 S m²mol^-1
3. 124 S cm² mol^-1
4. 124 S m² mol^-1

18. Given below are two statements:

Assertion (A):	Molar conductivity increases with a decrease in concentration.
Reason (R):	For strong electrolytes, $Λ_m$ increases slowly with dilution and can be represented by the equation: $\Lambda_m=\Lambda_m^0-A c^{1 / 2}$

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

19. Consider the given two statements:

Assertion(A):	$\mathrm{E^0_{cell}}$ = 0 for a chloride ion concentration cell.
Reason(R):	For this concentration cell, the equation is given by: $E_{\mathrm{cell}}=\frac{R T}{n F} \ln \left(\frac{\left[\mathrm{Cl}^{-}\right]_{\mathrm{LHS}}}{\left[\mathrm{Cl}^{-}\right]_{\mathrm{RHS}}}\right) $

1.	Both (A) and (R) are True and (R) is the correct explanation of (A)
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	(A) is False but (R) is True.

20. Given below are two statements:

Assertion (A):	1 coulomb of electricity deposits 1 g-equivalent of substance.
Reason (R):	1 Faraday is the charge on 1 mole of electricity.

1.	Both (A) and (R) are True, and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True, but (R) is not the correct explanation of (A).
3.	(A) is True, but (R) is False.
4.	(A) is False, but (R) is True.

21.

Find the emf of the cell in which the following reaction takes place at 298 K:
$\mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) $
$\small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=1.05 \mathrm{~V}; \dfrac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059} )$

1.	1.05 V	2.	1.0385 V
3.	1.385 V	4.	0.9615 V

22. Given below are half-cell reactions:
$\text{MnO}_{4}^{-}+8 \text{H}^{+}+5 \text{e}^{-} \rightarrow \text{Mn}^{2+}+4 \text{H}_{2} \text{O}, $
$ \text{E}_{\text{Mn}^{2+}}^{\circ} / \text{MnO}_{4}^{-}=-1.510 \text{ V} $
$ \frac{1}{2} \text{O}_{2}+2 \text{H}^{+}+2 \text{e}^{-} \rightarrow \text{H}_{2} \text{O}, $
$ \text{E}_{\text{O}_{2} / \text{H}_{2} \text{O}}^{\circ}=+1.223 \text{ V}$
Will the permanganate ion, $\text{MnO}_{4}^{-}$ , liberate $\text{O}_{2}$ from water in the presence of an acid?
1. No, because $\text{E}_{\text {cell }}^{\circ}=-2.733 \text{ V}$
2. Yes, because $\text{E}_{\text {cell }}^{\circ}=+0.287 \text{ V}$
3. No, because $\text{E}_{\text {cell }}^{\circ}=-0.287 \text{ V}$
4. Yes, because $\text{E}_{\text {cell }}^{\circ}=+2.733 \text{ V}$

23.

Consider the following cell:
$Pt, H_2|H^+||H^+|H_2, Pt~~, $
If a solution of pH = 3 is kept at the cathode and a solution of pH = 5 is kept at the anode, then $E_{cell} $ at 25 °C will be:
1. –0.059 V
2. +0.059V
3. +0.118 V
4. –0.118 V

24. Given below are some reactions. The reaction which is not feasible is
1. $2KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2 \uparrow$
2. $2KCl + I_2 \rightarrow 2KI + Cl_2 \uparrow$
3. Both 1 and 2 are not feasible
4. $2KI + Cl_2 \rightarrow 2KCl + I_2$

25. When 50% $H_2SO_4$ solution is electrolysed using inert electrodes, the products formed at anode and cathode, respectively, are
1. $H_2 ~and ~O_2$
2. $O_2 ~and~H_2O_2$
3. $H_2O_2 ~and~ H_2$
4. $O_2 ~and ~H_2$

26. When $CuSO_4$ solution using copper electrodes is electrolysed, pH of the solution
1. Increases
2. Decreases
3. Remains the same
4. Firstly increases and then decreases

27. Consider the following:
Cl₂| Cl^-|| Cl^-| Cl₂
(1atm) (C₁) (C₂) (1 atm)
For spontaneous cell, which of the following condition, is correct?
1. C₁> C₂
2. C₁ <C₂
3. C₁ = C₂
4. All of the above

28. The number of Faradays required for the evolution of 22.4 litres O₂ gas at NTP from the electrolysis of acidulated water are:
1. 1F
2. 2F
3. 3F
4. 4F

29. The molar conductivity of 0.05 M NH₄Cl is 20 S cm² mol^-1. The molar conductivities of $NH^+_4$ and $Cl^-$ ions at infinite dilution are 74 S cm² mol^-1 and 26 S cm² mol^-1, respectively. The dissociation constant of NH₄Cl will be:

1.	$2.5 \times 10^{-3}$	2.	$2 \times 10^{-3}$
3.	$2.5 \times 10^{-4}$	4.	$2 \times 10^{-4}$

30. Consider the following cell:
Ag | AgCl || $Cl^-~(C_1)$, AgCl | Ag.
The solubility product of AgCl is K_sp. The E_cell of the above cell will be ($2.303 RT \over F$ = 0.059)
1. $\frac{0.059}{2} \log \frac{C_{1}}{\sqrt{K_{s p}}}$
2. $\frac{0.059}{1} \log \frac{C_{1}}{\sqrt{K_{s p}}}$
3. $\frac{0.059}{2} \log \frac{K_{sp}}{{C_{1}}}$
4. $\frac{0.059}{1} \log \frac{\sqrt{K_{s p}}}{{C_{1}}}$

31. Consider the following cells:
Cell-1 $\rightarrow$ Zn | Zn²⁺ || Cu²⁺ | Cu
Cell-2 $\rightarrow$ Cu | Cu²⁺ || Zn²⁺ | Zn
$\small\left(E_{\mathrm{Cu}^{2+}/\mathrm{Cu}}^{o}=+0.34 \mathrm{~V};~ E_{\mathrm{Zn}^{2+}}^{o} /_{\mathrm{Zn}}=-0.76 \mathrm{~V};~\left[Z \mathrm{n}^{2+}\right]=1 ~\mathrm{M}\right)$
The maximum approximate concentration of [Cu²⁺] for the working of cell-2 would be:
1. 10^-15 M
2. 10^-25M
3. 10^-37 M
4. Cell-2 cannot work at any concentration of [Cu²⁺]

32. When a CuSO₄ solution using copper electrodes is electrolyzed, the incorrect statement among the following is:
1. The weight of the cathode increases.
2. O₂ gas is evolved at the anode.
3. The weight of the anode decreases.
4. pH of the solution remains the same.

33. Which of the following is a feasible reaction?
1. 2KCl + Br₂ $\rightarrow$ 2KBr + Cl₂
2. 2KBr + I₂  $\rightarrow$ 2KI + Br₂
3. 2KClO₃ + I₂  $\rightarrow$ 2KIO₃+ Cl₂
4. 2KIO₃ + Br₂  $\rightarrow$ 2KBrO₃ + l₂

34. Which metal evolves hydrogen gas when reacted with dilute HNO₃?

1.	Mn	2.	Zn
3.	Cu	4.	Fe

35.

For the following cell with hydrogen electrodes at two different pressures p₁ and p_{2 ,} then the emf is given by:
Pt(H₂) | H⁺(aq) |Pt (H₂)
p₁ 1M p₂

1.	$\frac{R T}{F} \log _{e} \frac{P_{1}}{p_{2}}$	2.	$\frac{R T}{2F} \log _{e} \frac{P_{1}}{p_{2}}$
3.	$\frac{R T}{F} \log _{e} \frac{P_{2}}{p_{1}}$	4.	$\frac{R T}{2F} \log _{e} \frac{P_{2}}{p_{1}}$

36.

The decreasing order of electrical conductivity of the following aqueous solutions is :
0.1 M Formic acid (A),
0.1 M Acetic acid (B),
0.1 M Benzoic acid (C)
1. A > B > C
2. A > C > B
3. C > B > A
4. C > A > B

37.

The value of E_cell in the reaction below will be:
$\small{Pt(s)|Br^{-}(0.010 \ M)|Br_{2}(l) \ ||H^{+}(0.030 \ M)|H_{2}(g)(1 \ bar)|Pt(s)}$
$E_{Br^{-}/Br_{2}}^{o} \ = \ -1.09 \ V$
1. +1.298 V

2. –1.398 V

3. –1.298 V

4. –1.198 V

38.

In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at the cathode while with Hg cathode it forms sodium amalgam because:

1.	Hg is more inert than Pt
2.	More voltage is required to reduce H⁺ at Hg than at Pt
3.	Na is dissolved in Hg while it does not dissolve in Pt
4.	The concentration of H⁺ ions is larger when the Pt electrode is taken

39.

For the disproportionation of copper:
2Cu⁺ → C u²⁺ + C u $,$ $E °$ is:
(Given $E °$ for Cu⁺²/Cu is 0.34 V & Eº for Cu⁺²/Cu⁺is 0.15 V )
1. 0.49 V
2. – 0.19 V
3. 0.38 V
4. – 0.38 V

40.

Given below are two statements:

Assertion (A):	$E^\circ$_{Ag⁺/ Ag} increases with an increase in the concentration of Ag⁺ ions.
Reason (R):	$E^\circ$_{Ag⁺/ Ag} has a positive value.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

41.

The incorrect statement about an inert electrode in a cell is:

1.	It does not participate in the cell reaction.
2.	It provides a surface either for oxidation or for the reduction reaction.
3.	It provides a surface for the conduction of electrons.
4.	It provides a surface for redox reaction.

42.

One liter of 0.5 M KCl solution is electrolyzed for one minute in a current of 1.608 mA. Considering 100 % efficiency, the pH of the resulting solution will be :

1.	Seven (7)	2.	Nine (9)
3.	Eight (8)	4.	Ten (10)

43.

Equivalent conductivity of ${BaCl}_{2}, H_{2} {SO}_{4} and HCl are x_{1}, x_{2} and x_{3} {Scm}^{- 1} {eq}^{- 1}$ at infinite dilution. If conductivity of saturated ${BaSO}_{4}$ solution is x ${Scm}^{- 1}, then K_{sp} of {BaSO}_{4}$ is:
(1) $\frac{500 x}{(x_{1} + x_{2} - 2 x_{3})}$
(2) $\frac{10^{6} x^{2}}{{(x_{1} + x_{2} - 2 x_{3})}^{3}}$
(3) $\frac{2.5 \times 10^{5} x^{2}}{{(x_{1} + x_{2} - x_{3})}^{2}}$
(4) $\frac{0.25 x^{2}}{{(x_{1} + x_{2} - x_{3})}^{2}}$

44.

A fuel cell develops an electrical potential from the combustion of butane at 1 bar and 298 K
C₄H₁₀(g) + 6.5O₂(g) → 4 CO₂(g) + 5H₂O(l); E^o of a cell is:
(Given $\Delta G^{o}$ $= - 2746 k J / m o l e$ )
1. 4.74 V
2. 0.547 V
3. 4.37 V
4. 1.09 V

45.

Consider the reaction given below:
$2 {CH}_{3} {COO}^{-} \to C_{2} H_{6} (g) + 2 {CO}_{2} (g) + 2 e^{-}$
The electrolysis of acetate solution produces ethane.
The current efficiency of the process is 80%.
What volume of gases would be produced at 27 $° C$ and 740 torr,
if the current of 0.5 amp is passed through the solution for 96.45 min?
1. 6.0 L
2. 0.60 L
3. 1.365 L
4. 0.91 L

46.

The specific conductivity of a saturated solution of KI₃ is 4.59 × 10^-6 ohm^-1 cm^-1 and it's molar conductance is 1.53 ohm^-1 cm² mol^-1. The K_sp Of KI₃ will be :
1. 4 x 10^-12
2. 27 x 27 x 10^-9
3. 9 x 10^-6
4. 4 x 10^-6

47.

In which electrolysis pH of solution decreases?
1. NaCl solution using Pt electrodes
2. ${CuSO}_{4}$ solution using Pt electrodes
3. ${CuSO}_{4}$ solution using Cu electrodes
4. All of these

48.

Equivalent conductance of saturated $\mathrm {BaSO}_4$ solution is $400 \mathrm { ~ohm}^{-1}$ $\mathrm {cm}^2$ $\mathrm { ~equivalent}^{-1}$ and it's specific conductance is $8 \times 10^{-5} \text { ohm}^{-1} \text {cm}^{-1}$ ; hence solubility product $K_{sp}$ of $\mathrm {BaSO}_4$ is :
1. $4 \times 10^{-8} \text {M}^2$
2. $1 \times 10^{-8} \text {M}^2$
3. $2 \times 10^{-4} \text {M}^2$
4. $1 \times 10^{-4} \text {M}^2$

49.

Consider the following Galvanic cell.

By what value the cell voltage change when concentration of ions in anodic and cathodic compartments both increased by a factor of 10 at 298
1. +0.0591
2. -0.0591
3. -0.1182
4. 0

50.

For which of these electrodes will the reduction potential vary with pH?
l.   ${AmO}_{_{2}}^{2^{+}} / {AmO}_{2}^{+}$
ll.   ${AmO}_{_{2}}^{2^{+}} / {Am}^{4 +}$
lll.   ${Am}^{4 +} / {Am}^{2 +}$
1. l only
2. ll only
3. l and ll only
4. l, ll and lll only

51.

What is the standard Gibbs free energy change (ΔG° in kJ/mol) for a Daniell cell with a standard cell potential (E°cell) of 1.1 V, when 2 moles of Zn(s) are oxidized at 298 K?

1.	–212.3	2.	–106.2
3.	–424.6	4.	–53.1

52.

Zinc gives H₂ with H₂SO₄ and HCl but not with HNO₃
because
1. Zinc acts as oxidising agent when reacts with
HNO₃
2. HNO₃ is a weaker acid then H₂
SO₄ and HCl
3. In electrochemical series zinc is above
hydrogen
4. is reduced is preference to hydronium ion

53.

Given that
$I_{2} + 2 e^{-} \to 2 I^{-}; E^{o} = 0.54 V$
${Br}_{2} + 2 e^{-} \to 2 {Br}^{-}; E^{o} = 1.09 V$
1. I¯ ions will be able to reduce bromine
2. Br¯ ion will be able to reduce iodine
3. Iodine will be able to reduce bromide ions
4. Bromine will be able to reduce iodide ions

54.

The ionization constant of a weak acid is $1.6 \times 10^{- 5}$ and the molar conductivity at infinite dilution is $380 \times 10^{- 4}$ S $m^{2} m o l^{- 1}$ . If the cell constant is 0.01 $m^{- 1}$ then conductance of 0.01 M acid solution is:
(1) $1.52 \times 10^{- 5} S$
(2) 1.52 S
(3) 1.52 $\times 10^{- 3}$ S
(4) $1.52 \times 10^{- 4} S$

55.

Given the cell: $\mathrm{Cd}(s)\left|\mathrm{Cd}(\mathrm{OH})_2(s)\right| \mathrm{NaOH}(a q, 0.01 M) \mid H_2(g), 1 \text { bar } \mid P t(s)$
with E_cell = 0.0 V. If E°_Cd²⁺lCd = -0.39 V, then Ksp of Cd(OH)₂ is:
1. 0.1
2. $10^{- 13}$
3. $10^{- 15}$
4. None of these

56.

A fuel cell develops an electrical potential from the coombustion of butane at 1 bar and 298 K
$C_{4} H_{10} (g) + 6.5 O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l);$
$∆_{r} G^{°} = - 2746 k J / m o l$
What is $E^{°}$ of a cell?
(1) 4.74 V
(2) 0.547 V
(3) 4.37 V
(4) 1.09 V

57.

108 g fairly concentrate solution of $A g N O_{3}$ is electrolyzed using 0.1 F of electricity. The weight of resulting solution is:
(1) 94 g
(2) 11.6 g
(3) 96.4 g
(4) None of these

58.

Pt | Cl₂ (P₁) | HCl (0.1 M) | Pt | Cl₂ (P₂) ; cell reaction will be spontaneous if :
1. P₁ = P₂ 2. P₁ > P₂
3. P₂ > P₁ 4. P₁ = P₂ = 1 atm

59.

Molar conductance of 0.1 M acetic acid is 7 ohm^–1 cm² mol^–1 .
If the molar conductance of acetic acid at infinite dilution is 380.8 ohm^–1 cm² mol^–1,
the value of dissociation constant will be -
1. 226 × 10^–5 mol dm^–3
2. 1.66 × 10^–3 mol dm^–1
3. 1.66 × 10^–2 mol dm^–3
4. 3.442 × 10^–5 mol dm^–3

60.

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to:

1.	increase in ionic mobility of ions
2.	100% ionization of electrolyte at normal dilution
3.	increase in both, i.e, number of ions and ionic mobility of ions
4.	increase in the number of ions

61.

What is the reduction potential at pH = 14 for the Cu²⁺/Cu couple?
[Given: $E_{Cu^{2+}/Cu}^{o}$ = 0.34 V; $K_{sp}~\text Cu \text({OH})_2$ = 1×10^-19]

1.	0.34 V	2.	-0.34 V
3.	0.22 V	4.	-0.22 V

62.

The volume of gases liberated at STP when a charge of 2F is passed
through aqueous solution of sodium phosphate, is :
1. 11.2L
2. 44.8L
3. 33.6L
4. 22.4L

63.

Value of $\land_{m}^{0}$ for  $SrCl_{2}$ (strong electrolyte) in water at 25°C from the data below is:

Conc. (mol/litre)	0.25	1
$\land_{m} \Omega^{- 1 } c m^{2 } m o l^{- 1}$	260	250

1. 270 Ω^-1 cm² mol^-1
2. 260 Ω^-1 cm² mol^-1
3. 250 Ω^-1 cm² mol^-1
4. 255 Ω^-1 cm² mol^-1

64.

The calomel electrode is reversible with respect to-
1. Mercury
2. $H^{+}$
3. $H g^{2 +}$
4. $C l^{-}$

65.

If ${E^{0}}_{A u^{+} / A u}$ is 1.69 V and ${E^{0}}_{A u^{3 +} / A u}$ is 1.40 V, then ${E^{0}}_{A u^{+ 3} / A u^{1 +}}$ will be :
1. 0.19 V
2. 2.945 V
3. 1.255 V
4. None of the above

66.

Standard electrode potential data are useful for understanding the suitability of an oxidant in aredox titration. Some half cell reactions and their standard potential are given below

${MnO}_{4}^{-} (aq) + 8 H^{+} (aq) + 5 e^{-} \to {Mn}^{2 +} (aq) + 4 H_{2} O (l); E ° = 1.51 V$
${Cr}_{2} O_{7} {}_{2 -}(aq) + 14 H^{+} (aq) + 6 e^{-} \to 2 {Cr}^{3 +} (aq) + 7 H_{2} O (l); E ° = 1.38 V$

{Fe}^{3 +} (aq) + e^{-} \to {Fe}^{2 +} (aq); E ° = 0.77 V

${Cl}_{2} (g) + 2 e^{-} \to 2 {Cl}^{-} (aq); E ° = 1.40 V$
Identify the only incorrect statement regarding the quantitative estimation of aqueous $Fe (NO$
${MnO}_{4}^{-}$ can be used in aqueous $HCl$
${Cr}_{2} O_{7}^{2 -}$ can be used in aqueous $HCl$
${MnO}_{4}^{2 -}$ can be used in aqueous $H_{2} {SO}_{4}$
${Cr}_{2} O_{7}^{2 -}$ can be used in aqueous $H_{2} {SO}_{4}$

67.

Zinc gives H₂ with H₂SO₄ and HCI but not with HNO₃ because
(1) Zinc acts as oxidizing agent when react with HNO₃
(2) HNO 3 is a weaker acid then H₂SO₄ and HCI
(3) In electrochemical series, the zine is above hydrogen
(4) NO $\bar{3}$ is reduced is a preference to hydronium ion

68.

During electrolysis of conc. H₂SO₄, perdisulphuric acid (H₂S₂O₈), and O₂
form in equimolar amount. The amount of H₂ that will form simultaneously will be :
1. Thrice that of O₂ in moles.
2. Twice that of O₂ in moles.
3. Equal to that of O₂ in moles.
4. Half of that of O₂ in moles.

69.

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.5x10⁴ A of
current is passed through molten Al₂O₃ for 6 h,what mass of aluminium is produced ?
(Assume 100% current efficiency, at. mass of Al = 27 g mol^-1)
1. 9.0 x 10³ g
2. 9.1 x 10⁴ g
3. 2.4 x 10⁵ g
4. 1.3 x 10⁴g

70.

The quantity of electricity required to reduce 12.3 g of nitrobenzene to aniline with 50 % current efficiency is:
1. 1 F
2. 0.6 F
3. 0.5 F
4. 1.2 F

71.

Three Faradays of electrical charge are passed consecutively through four separate electrolytic cells containing aqueous solutions of AgNO₃, CuSO₄, Al(NO₃)₃, and NaCl. What will be the molar ratio of the respective metals deposited at each cathode?

1.	1 : 2 : 3 : 1	2.	6 : 3 : 2 : 6
3.	6 : 3 : 0 : 0	4.	3 : 2 : 1 : 0

72.

If an iron rod is dipped in CuSO₄ solution, then:
1. Blue colour of the solution turns red.
2. Brown layer is deposited on iron rod.
3. No change occurs in the colour of the solution.
4. None of the above.

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1.	\(K_a \times (\wedge^\circ _M )^2\)	2.	\(K_a \times {1 \over (\wedge^\circ _M )^3}\)
3.	\(K_a \times {1 \over (\wedge^\circ _M )^2}\)	4.	\(K_a\times (\wedge^\circ _M )^3 \)

1.	\(1.2 \times 10^{-43}\)	2.	\(2.4 \times 10^{-73}\)
3.	\(6.3 \times 10^{-92}\)	4.	\(1.5 \times 10^{-62}\)

Statement I	For \(\mathrm{Kl},\) molar conductivity increases steeply with dilution.
Statement II	For carbonic acid, molar conductivity increases slowly with dilution.

1.	\(\small{\mathrm{Cd}_{(\mathrm{s})}+\mathrm{NiO}_{2(\mathrm{~s})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{Cd}(\mathrm{OH})_{2(\mathrm{~s})}+\mathrm{Ni}(\mathrm{OH})_{2(\mathrm{~s})}}\)
2.	\(\small {Cd_{(s)} + NiO_{2{(s)}} + 2OH^-_{(aq)} \rightarrow Ni{(s)} + Cd(OH)_{2{(s)}}}\)
3.	\(\small {Ni_{(s)}+ Cd(OH)_{2{(s)} }\rightarrow Cd_{(s)}+ Ni(OH)_{2{(s)}}}\)
4.	\(\small {Ni(OH)_{2(s)}+Cd(OH)_{2(s)} \rightarrow Ni_{(s)} + Cd_{(s)}+2H_2O(l)}\)

1.	\(I^-(aq) \|I_2(s) \|\| Br_2(l) \|Br^-(aq) \)
2.	\(Zn(s) \| Zn^{2+} (aq) \|\| Pb^{2+} (aq) \| Pb(s) \)
3.	\(Pt,H_2(g) \|H_2O(l) \| OH^-(aq) \|\|O_2(g) \|OH^- (aq), Pt\)
4.	\(Ag(s) \| Ag^+ (aq) \|\| Ag^+ (aq) \|Ag(s) \)

Assertion(A):	\(\mathrm{E^0_{cell}}\) = 0 for a chloride ion concentration cell.
Reason(R):	For this concentration cell, the equation is given by: \(E_{\mathrm{cell}}=\frac{R T}{n F} \ln \left(\frac{\left[\mathrm{Cl}^{-}\right]_{\mathrm{LHS}}}{\left[\mathrm{Cl}^{-}\right]_{\mathrm{RHS}}}\right) \)

1.	\(2.5 \times 10^{-3}\)	2.	\(2 \times 10^{-3}\)
3.	\(2.5 \times 10^{-4}\)	4.	\(2 \times 10^{-4}\)

1.	\(\frac{R T}{F} \log _{e} \frac{P_{1}}{p_{2}}\)	2.	\(\frac{R T}{2F} \log _{e} \frac{P_{1}}{p_{2}}\)
3.	\(\frac{R T}{F} \log _{e} \frac{P_{2}}{p_{1}}\)	4.	\(\frac{R T}{2F} \log _{e} \frac{P_{2}}{p_{1}}\)

Assertion (A):	\(E^\circ\)_{Ag⁺/ Ag} increases with an increase in the concentration of Ag⁺ ions.
Reason (R):	\(E^\circ\)_{Ag⁺/ Ag} has a positive value.

Conc. (mol/litre)	0.25	1
\(\land_{m} \Omega^{- 1 } c m^{2 } m o l^{- 1}\)	260	250

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