1. In the electrolysis of molten \(\mathrm{Al}_2 \mathrm{O}_3\) with inert electrodes

(a) \(\mathrm{Al}\) is axidized at anode to \(\mathrm{Al}^{\mathrm{l}}\)

(b) \(\mathrm{O}_2\) gas is produced at anode

(c) \(\mathrm{O}^{-}\)is reduced at cathode

(d) \(\mathrm{O}\) is oxidised at anode

2. The number of electrons that have a total charge of 965 coulo mbs is

(a) \(6.022 \times 10^{23}\)

(b) \(6.022 \times 10^{22}\)

(c) \(6.022 \times 10^4\)

(d) \(3.011 \times 10^{\mathrm{as}}\)

3. The time required to produce \(2 \mathrm{~F}\) of electricity with a current of 2.5 amperes is

(a) \(13.4 \mathrm{~h}\)

(b) 1200 min

(c) \(50000 \mathrm{~s}\)

(d) \(1.5 \mathrm{~h}\)

4. The number of Faradays required to produce 0.5 mol of free metal from \(\mathrm{Al}^{\mathrm{H}}\) is

(a) 3

(b) 2

(c) 6

(d) 1.5

5. The number of coulombs necessary to deposit 1 g of potassium metal ( molar mass \(39 \mathrm{e} \mathrm{mol}^{-1}\) ) from \(\mathrm{K}^+\) ions is

(a) \(96500 \mathrm{C}\)

(b) \(1.93 \times 10^3 \mathrm{C}\)

(c) \(1237 \mathrm{C}\)

(d) \(2474 \mathrm{C}\)

6. The strongest oxidizing agent among the species \(\ln ^{3+}\left(\mathrm{E}^2=-1.34 \mathrm{~V}\right), \mathrm{Au}^{3+}\left(\mathrm{E}^2=1.4 \mathrm{~V}\right), \mathrm{H}_{\mathrm{g}^2+}\left(\mathrm{E}^2=\right.\) \(0.85 \mathrm{~V}), \mathrm{Cr} \mathrm{r}^j(\mathrm{E}=-0.74 \mathrm{~V})\) is

(a) \(\mathrm{Cr}^2\)

(b) \(\mathrm{Au}=\)

(c) \(\mathrm{Hg}^{2+}\)

(d) \(\ln ^{3-}\)

7. The value of constant in Nernat equation \(\mathrm{E}=\mathrm{E}^0-\frac{\text { constant }}{\mathrm{n}}\) in \(\mathbf{Q}\) at \(25^{\circ} \mathrm{C}\) is

(a) \(0.0592 \mathrm{mV}\)

(b) \(0.0592 \mathrm{~V}\)

(c) \(25.7 \mathrm{mV}\)

(d) \(0.0296 \mathrm{~V}\)

8. The reaction, \(2 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{Sn}^{t+}(\mathrm{aq}) \Longrightarrow \mathrm{Br}_2(\mathrm{I})\) \(+\operatorname{Sn}(\bar{s})\) with the standard potentiak. \(\mathbf{E}^0 \mathrm{Sn}=-0.114 \mathrm{~V}, \mathbf{E}^0 \mathrm{_Br}_2=+1.09 \mathrm{~V}\), is

(a) spontaneous in reverse direction

(b) spontaneous in forward direction

(c) at equilibrium

(d) nonspontaneous in reverse direction.

9. Daniel cell operates under nonstandard state conditions. If the equation of the cell reaction is multiplied by 2 then

(a) \(E\) and \(E^{\prime}\) remain unchanged

(b) E is doubled

(c) \(n\) remains unchanged in Nernst equation.

(d) \(\mathrm{Q}\) is halved in Nernst equation.

10. Consider the cell, \(\mathrm{Pt}\left|\mathrm{H}_2(\mathrm{~g})\right| \mathbf{H}^{+}{ }_{(2 q)} \| \mathbf{I}(\mathrm{aq}) \mid\) \(I_2(\mathrm{~s})\). If the standard cell potential is \(0.54 \mathrm{~V}\) then the standard potential for cathode half reaction will be

(a) \(0 \mathrm{~V}\)

(b) \(-0.54 \mathrm{~V}\)

(c) \(+0.54 \mathrm{~V}\)

(d) \(1.08 \mathrm{~V}\)

11. Consider the cell \(\mathrm{Pt} \mid \mathrm{Cl}_2\) (g) \(\mid \mathrm{HCl}(\mathrm{aq}) \| \mathrm{HBr}\) (aq) \(\mid \mathrm{Br}_2\) (I) \(\mid \mathrm{Pt}\). If concentration of \(\mathrm{HCl}\) is increased, the cell potential will

(a) increase

(b) decrease

(c) remain the same

(d) become maximum

12. The standard potential for the cell reaction \(2 \mathrm{T1}(\mathrm{s})+\mathrm{Hg}^{2+}(1 \mathrm{M}) \longrightarrow 2 \mathrm{Ti}^{+}(1 \mathrm{M})+\mathrm{Hg}(\mathrm{l})\) where \(\mathrm{E}_{\mathrm{T} 1}^0=-0.34 \mathrm{~V}, \mathrm{E}_{\mathrm{H}_2}^0=0.86 \mathrm{~V}\) is

(a) \(0.52 \mathrm{~V}\)

(b) \(-0.52 \mathrm{~V}\)

(c) \(-1.2 \mathrm{~V}\)

(d) \(+1.2 \mathrm{~V}\)

13. \(\Delta \mathrm{G}^0\) for the reaction

\(\mathrm{Ag}^{+}(\mathrm{aq})+1 / \mathrm{H}_2(\mathrm{~g}) \longrightarrow \mathrm{H}^{+}(\mathrm{aq})+\mathrm{Ag}(\mathrm{s})\), where standard potential for silver half cell reaction is \(0.8 \mathrm{~V}\), will be

(a) \(-77.2 \mathrm{~kJ}\)

(b) \(+77.2 \mathrm{~kJ}\)

(c) \(154.4 \mathrm{~kJ}\)

(d) \(-38.6 \mathrm{~kJ}\)

14. The following reaction occurs in a galvanic cell

$$

2 \mathrm{Cu}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Cu}

$$

If \(\mathrm{E}_{\mathrm{eu}^{+}}^0, \mathrm{Cua}^2+=+0.16 \mathrm{~V}\) and \(\mathrm{E}_{\mathrm{Cut} i \mathrm{ca}}^0=0.52 \mathrm{~V}\), the standard cell potential will be

(a) \(0.68 \mathrm{~V}\)

(b) \(0.36 \mathrm{~V}\)

(c) \(-0.36 \mathrm{~V}\)

(d) \(-0.68 \mathrm{~V}\)

15. The SI unit of molar conductivity is

(a) \(\mathrm{S} \mathrm{cm}^2 \mathrm{~mol}^{-1}\)

(b) \(\mathrm{S} \mathrm{dm}^2 \mathrm{~mol}^{-1}\)

(c) \(\mathrm{S} \mathrm{m}^2\)

(d) \(\mathrm{S} \mathrm{m}^2 \mathrm{~mol}^{-1}\)

16. Consider the following half reactions and choose the correct alternative

(i) \(\mathrm{Cl}_2\) (g) \(+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Cl}^{-}\)(aq) \(\mathrm{E}^0=1.36 \mathrm{~V}\)

(ii) \(\mathrm{Br}_2(\mathrm{I})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Br}^{-}\)(aq) \(\quad \mathrm{E}^0=1.07 \mathrm{~V}\)

(iii) \(\mathrm{I}_2(\mathrm{~s})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{I}\)-(aq) \(\quad \mathrm{E}^0=0.53 \mathrm{~V}\)

(a) \(\mathrm{Br}_2\) cannot oxidize \(\mathrm{I}^{-}\)

(b) \(\mathrm{Cl}_2\) can oxidize \(\mathrm{Br}\) but not \(\mathrm{I}^{-}\)

(c) \(\mathrm{I}_2\) can oxidize \(\mathrm{Cl}^{-}\)

(d) \(\mathrm{Br}_2\) can oxidize \(\mathrm{I}^{-}\)but not \(\mathrm{Cl}^{-}\)

17. Maximum standard emf will be delivered by the cell consisting of the half cells

(a) \(\mathrm{F}^{-} \mid \mathrm{F}_2\) and \(\mathrm{Br} \mid \mathrm{Br}^2\)

(b) \(\mathrm{F}^{-} \mid \mathrm{F}_2\) and \(\mathrm{Li}^{+} \mid \mathrm{Li}\)

(c) \(\mathrm{Li}^{+} \mid \mathrm{Li}\) and \(\mathrm{Ca}^{2+} \mid \mathrm{Ca}\)

(d) \(\mathrm{Br} \mid \mathrm{Br}\), and \(\mathrm{Au}^{+} \mid \mathrm{Au}\).

18. During electrolysis, \(2 \mathrm{~A}\) current is passed through an electrolytic solution for \(965 \mathrm{~s}\). The number of moles of electrons passed will be

(a) 0.02

(b) 0.01

(c) 200

(d) 0.037

19. The same quantity of electricity is passed through two cells one containing \(\mathrm{AlCl}_3\) solution and the other containing \(\mathrm{ZnCl}_2\) solution. If 0.04 mole of \(\mathbf{A l}\) is produced in the first cell, the number of moles of \(\mathrm{Zn}\) produced in the second cell will be

(a) 0.08

(b) 0.0267

(c) 0.06

(d) 0.02

20. \(\mathbf{E}^0\) of an electrode half reaction is related to \(\Delta G^0\) by the equation, \(E^*=-\Delta G^0 / n F\). If the amount of \(\mathrm{Ag}^{+}\)in the half reaction

\(\mathbf{A g}^{+}+\mathrm{e}^{-} \longrightarrow \mathbf{A g}\) is tripled then

(a) \(\mathrm{n}\) is tripled

(b) \(\Delta G^{\circ}\) reduces to one third

(c) \(\mathrm{E}^0\) reduces to one third

(d) all the above

21. Electrolysis involves oxidation and reduction respectively at

(a) anode and cathode

(b) cathode and anode

(c) at both the electrodes

(d) none of these

22. When electricity is allowed to pass then which of the following is decomposed?

(a) Urea

(b) Glucose

(c) Ethyl alcohol

(d) \(\mathrm{AgNO}_3\)

23. The amount of ion discharged during electrolysis is not directly proportional to

(a) Resistance

(b) Time

(c) Current

(d) Chemical equivalent

24. During electrolysis the species discharged at cathode are

(a) ions

(b) cations

(c) anions

(d) all of these

25. Which of the following is not non-electrolyte?

(a) Acetic acid

(b) Glucose

(c) Ethanol

(d) Urea

26. The electric charge required to deposit one gram equivalent of an element is

(a) one ampere current

(b) 96500 coulombs per second

(c) charge on one mole of electrons

(d) both b and c

27. Which of the following is not a strong electrolyte?

(a) aqueous caustic potash

(b) acetic acid

(c) dil hydrochloric acid

(d) fused \(\mathrm{NaCI}\)

28. Which of the following is not a good conductor of electricity?

(a) \(\mathrm{NaCl}\) (Molten)

(b) \(\mathrm{NaCl}(\mathrm{aq})\)

(c) \(\mathrm{NaCl}(\mathrm{s})\)

(d) Silver metal

29. The number of Faradays required to produce \(0.5 \mathrm{~mol}\) of free metal from \(\mathrm{Al}^{3+}\) is

(a) 3

(b) 2

(c) 6

(d) 1.5

30. Prevention of corrosion of iron by Zn coating is called?

(a) Galvanization

(b) Cathodic protection

(c) Electrolysis

(d) Photoelectrolysis

31. In voltaic cell the two half cells are always connected by

(a) Salt bridge

(b) Porous partition

(c) Porous pot

(d) Any of these

32. The number of coulombs necessary to deposit \(\lg\) of potassium metal (molar mass \(39 \mathrm{~g} \mathrm{~mol}^{-1}\) ) from \(\mathrm{K}^{+}\)ions is

(a) \(96500 \mathrm{C}\)

(b) \(1.93 \times 10^5 \mathrm{C}\)

(c) \(1237 \mathrm{C}\)

(d) \(2474 \mathrm{C}\)

33. Which of the following metals can deposit copper from copper sulphate solution?

(a) Mercury

(b) Iron

(c) Gold

(d) Platinum

34. During working of Daniell cell

(a) Zn rod grows in size

(b) Cu rod grows in size

(c) \(\mathrm{Zn}\) rod reduces in size

(d) both \(\mathrm{b}\) and \(\mathrm{c}\)

35. For SHE arbitrarily

(a) \(\mathrm{Ps}_{\mathrm{S}}>\mathrm{P}_{\mathrm{O}}\)

(b) \(\mathrm{P}_{\mathrm{o}}>\mathrm{P}_{\mathrm{s}}\)

(c) \(\mathrm{P}_{\mathrm{s}}=\mathrm{P}_{\mathrm{O}}\)

(d) none of them

36. An electrode can be in a state of

(a) solid

(b) liquid

(c) gas

(d) all of these

37. When a gas like \(\mathrm{H}_2\) or \(\mathrm{Cl}_2\) are to be used as an electrode it is incorporated with

(a) The glass jacket

(b) Platinum as an inert electrode

(c) Al metal

(d) Another gas electrode

Pt The reduction reaction taking place at the cathode will be

(a) \(\frac{1}{2} \mathrm{Cl}_2+\mathrm{e}^{-} \rightarrow \mathrm{Cl}^{-}\)

(b) \(\frac{1}{2} \mathrm{O}_{2(y)} \rightarrow \frac{1}{2} \mathrm{O}_2^{2-}+2 \mathrm{e}^{-}\)

(c) \(2 \mathrm{OH}^{-} \rightarrow \frac{1}{2} \mathrm{O}_{2(g)}+\mathrm{H}_2 \mathrm{O}+\mathrm{e}^{-}\)

(d) \(\mathrm{Cl}_2 \rightarrow 2 \mathrm{Cl}^{-}+2 \mathrm{e}^{-}\)

39. The single electrode potential depends upon following factor

(a) temperature

(b) nature of electrode

(c) conc. of the electrolyte

(d) all of these

40. The redox reaction during discharging of the lead accumulator is

(a) \(\mathrm{Pb} \rightarrow \mathrm{Pb}^{2+}+2 \mathrm{e}^{-}\)

(b) \(\mathrm{PbO}_2+\mathrm{H}^{+}+\mathrm{SO}_2+2 \mathrm{e}^{-} \rightarrow \mathrm{PbSO}_4+2 \mathrm{H}_2 \mathrm{O}\)

(c) \(\mathrm{Pb}_{(01}+\mathrm{PbO}_{200}+2 \mathrm{H}_2 \mathrm{SO}_{44=0} \rightarrow 2 \mathrm{PbSO}_{400}+2 \mathrm{H}_2 \mathrm{O}\)

(d) \(2 \mathrm{PbSO}_{400}+2 \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{Pb}_{40}+\mathrm{PbO}_{200}+2 \mathrm{H}_2 \mathrm{SO}_{400}\)

41. Daniel cell operates under nonstandard state conditions. If the equation of the cell reaction is multiplied by 2 then

(a) \(E\) and \(E^u\) remain unchanged

(b) \(\mathrm{E}\) is doubled

(c) n remains unchanged in Nemst equation.

(d) \(Q\) is halved in Nernst equation.

42. Which of the following metal can not liberate \(\mathrm{H}_2\) gas from dilute hydrochloric acid?

(a) \(Z \mathrm{n}\)

(b) \(\mathrm{Mg}\)

(c) Al

(d) Ag

43. Calomel electrode is an example of

(a) Indicator electrode

(b) Primary reference electrode

(c) Secondary reference electrode

(d) None of these

44. Lead accumulator acts as

(a) voltaic cell

(b) electrolytic cell

(c) both of these

(d) none of these

45. Accurate measurement of the emf of an electrochemical cell is done by

(a) voltmeter

(b) potentiometer

(c) galvanometer

(d) conductometer

46. Which of the following metals is most readily corrodes in moist air?

(a) Al

(b) \(\mathrm{Fe}\)

(c) both 'a' and 'b'

(d) None of these

47. The time in hours required for a current of ampere to decompose electrolytically \(18 \mathrm{~g}\) of \(\mathrm{H}_2 \mathrm{O}\)

(a) 9

(b) 18

(c) 36

(d) 54

48. In air galvanic cell during its working if suddenly the salt bridge is removed then the potential of the cell

(a) Remains same

(b) Increases to maximum

(c) Decreases half the value

(d) Drops to zero

49. In a saturated calomel electrode the KCI solution is saturated with

(a) only \(\mathrm{KCl}\)

(b) only calomel

(c) both \(\mathrm{KCl}\) and calomel

(d) none

50. The ECE of a metal is " \(E\) " the amount of the metal deposited by the passage of \(500 \mathrm{~m} /\) current through the solution for 4 minutes will be

(a) \(2000 \mathrm{E} \mathrm{g} / \mathrm{F}\)

(b) \(1200 \mathrm{E} \mathrm{g} / \mathrm{F}\)

(c) \(120 \mathrm{E} \mathrm{g} / \mathrm{F}\)

(d) \(2 \mathrm{E} \mathrm{g} / \mathrm{F}\)

51. Which one of the following statements is correct?

(a) During the electrolytic dissociation, the number of cations and anions obtained are always equal

(b) The electrolytic dissociation leads reduction in the number of particles in the solution

(c) The cations and anions do not reunite to give back neutral molecules

(d) The number of positive and negative ions are equivalent

52. The equivalent weights of the elements \(A, \mathbf{B}\) and \(C\) are in inereasing order. Their weights deposited in electroly tic cells by the same quantity of electricity are \(x\), \(y\) and \(w\) respectively. Then

(a) \(x>y>w\)

(b) \(\mathrm{x}=\mathrm{Y}=\mathrm{w}\)

(c) \(x<y<w\)

(d) \(\mathrm{x}>\mathrm{Y} \leqslant \mathrm{w}\)

53. The main function of the salt bridge is

(a) to allow ions to go from one half cell to another

(b) to provide link between two half cells

(c) to keep the emf of the cell positive

(d) to maintain electrical neutrality of the solutions in the two half cells

54. The SI unit of molar conductivity is

(a) \(\mathrm{S} \mathrm{cm}^2 \mathrm{~mol}^{-1}\)

(b) \(\mathrm{S} \mathrm{dm}^2 \mathrm{~mol}^{-1}\)

(c) \(\mathrm{S} \mathrm{m}^2\)

(d) \(\mathrm{S} \mathrm{m}^2 \mathrm{~mol}^{-1}\)

55. Out of \(\mathrm{Cu}, \mathrm{Ag}, \mathrm{Fe}\) and \(\mathrm{Zn}\), the metal which can displace all others from their salt solutions is

(a) Ag

(b) \(\mathrm{Cu}\)

(c) \(\mathrm{Zn}\)

(d) Fe

56. Molar conductivity of a solution is \(1.26 \times 10^{-2}\) \(\mathbf{Q}^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\). It is molarity is 0.01. Its specific conductivity will be

(a) \(1.26 \times 10^{-15}\)

(b) \(1.26 \times 10^{-3}\)

(c) \(1.26 \times 10^{-4}\)

(d) 0.0063

57. Molar ionic conductivities of a bivalent electrolyte are 57 and 73 . The molar conductivity of the solution will be

(a) \(130 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)

(b) \(65 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)

(c) \(260 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)

(d) \(187 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\)

58. A smuggler could not carry gold by chemically depositing iron on the gold surface since

(a) gold is denser

(b) iron rusts

(c) gold has higher reduction potential than iron

(d) gold has lower reduction potential than iron

59. On the basis of the information available for the reaction

$$

\begin{aligned}

& 4 / 3 \mathrm{Al}+\mathrm{O}_2 \rightarrow 2 / 3 \mathrm{Al}_2 \mathrm{O}_3 \\

& \Delta \mathrm{G}=-827 \mathrm{~kJ} / \mathrm{mol}

\end{aligned}

$$

of the minimum e.m.f. required to carry out electrolysis of \(\mathrm{Al}_2 \mathrm{O}_3\) is \(\left(\mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1}\right)\)

(a) \(8.56 \mathrm{~V}\)

(b) \(2.14 \mathrm{~V}\)

(c) \(4.28 \mathrm{~V}\)

(d) \(6.42 \mathrm{~V}\)

60. Several blocks of magnesium are fixed to the bottom of a ship to

(a) keep away the sharks

(b) make the ship lighter

(c) prevent action of water and salt

(d) prevent puncturing by under-sea rocks.