chapter 20 quiz - ibiokaare.com · _____ kj/mol. pb (s) + 2h+ (aq ... how many grams of cus are...

Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O

A) S4O62- B) Cr2O72- C) Cr3+ D) S2O32- E) H+

2) Which substance is serving as the reducing agent in the following reaction?

14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

A) Ni B) H2O C) Cr2O72- D) Ni2+ E) H+

3) __________ electrons appear in the following half-reaction when it is balanced.

S4O62- → 2S2O32-

A) 2 B) 4 C) 3 D) 1 E) 6

4) The balanced half-reaction in which dichromate ion is reduced to chromium(III) ion is a __________process.

5) The half-reaction occurring at the anode in the balanced reaction shown below is __________.

3MnO4- (aq) + 24H+ (aq) + 5Fe (s) → 3Mn2+ (aq) + 5Fe3+ (aq) + 12H

2O (l)

A) 2MnO4- (aq) + 12H+ (aq) + 6e- → 2Mn2+ (aq) + 3H2O (l)

B) Fe2+ (aq) → Fe3+ (aq) + e-

C) MnO4- (aq) + 8H+ (aq) + 5e- → Mn2+ (aq) + 4H2O (l)

D) Fe (s) → Fe3+ (aq) + 3e-

E) Fe (s) → Fe2+ (aq) + 2e-

1) __________ is reduced in the following reaction:

A) three-electron B) six-electron C) twelve-electronD) four-electron E) two-electron

E) salt bride, anode

6) In a voltaic cell, electrons flow from the __________ to the __________.A) anode, salt bridge B) cathode, anodeC) anode, cathode D) salt bridge, cathode

7) 1V = __________.A) 1 amp · s B) 1 J/C C) 96485 C D) 1 J/s E) 1 C/J

AIIMS,CBSE,AIPMT, AFMC,Bio.Tech & PMT, Contact :- 9438559863, Mail at :- [email protected],www.ibiokaare.com,compiled by AKB

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8) The more __________ the value of E°red, the greater the driving force for reduction.

Table 20.2Half-reaction E° (V)Cr3+ (aq) + 3e- → Cr (s) -0.74Fe2+ (aq) + 2e- → Fe (s) -0.440Fe3+ (aq) + e- → Fe2+ (s) +0.771Sn4+ (aq) + 2e- → Sn2+ (aq) +0.154

9) The standard cell potential (E°cell) for the voltaic cell based on the reaction below is __________ V.

Cr (s) + 3Fe3+ (aq) → 3Fe2+ (aq) + Cr3+ (aq)

A) -1.45 B) +1.51 C) +1.57 D) +2.99 E) +3.05

10) The standard cell potential (E°cell) of the reaction below is +0.126 V. The value of ΔG° for the reaction is__________ kJ/mol.

Pb (s) + 2H+ (aq) → Pb2+ (aq) + H2 (g)

A) -24 B) +24 C) -12 D) +12 E) -50

11) Galvanized iron is iron coated with __________.A) phosphate.B) magnesium.C) iron oxide.

D) zinc.E) chromium.

A) negative B) extensive C) endothermic D) exothermic E) positive

12) Corrosion of iron is retarded by __________.A) high pH conditions

E) both the presence of salts and low pH conditions

B) the presence of saltsC) low pH conditionsD) both the presence of salts and high pH conditions

13) How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr3+

A) 5.77 B) 17.3 C) 1.92 D) 346 E) 115

using acurrent of 35.2 amps in an electrolyte cell __________ ?

14) How many grams of CuS are obtained by passing a current of 12 A through a solution of CuSO4 for 15minutes __________ ?A) 3.6 B) 1.8 C) 14 D) 7.1 E) 0.016

15) Which of the following reactions is a redox reaction?(a) K2CrO4 + BaCl2 → BaCrO4 + 2KCl(b) Pb22+ + 2Br- → PbBr(c) Cu + S → CuS

A) (a) only B) (b) only C) (c) only D) (b) and (c) E) (a) and (c)


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16) Which transformation could take place at the anode of an electrochemical cell?A) F2 toF-

B) Cr2O72- → Cr2+

C) O2 to H2O

D) HAsO2 to As

E) None of the above could take place at the anode.

17) The purpose of the salt bridge in an electrochemical cell is to __________.A) maintain electrical neutrality in the half-cells via migration of ions.B) provide a means for electrons to travel from the cathode to the anode.C) provide oxygen to facilitate oxidation at the anode.D) provide a means for electrons to travel from the anode to the cathode.E) provide a source of ions to react at the anode and cathode.

18) Which transformation could take place at the cathode of an electrochemical cell?A) Br2 → BrO3-

B) NO → HNO2C) HSO4- → H2SO3D) MnO2 → MnO4-

E) Mn2+ → MnO4-19) Which one of the following types of elements is most likely to be a good oxidizing agent?

A) halogensB) alkaline earth elementsC) lanthanides

D) transition elementsE) alkali metals

20) Which one of the following is the best oxidizing agent ?A) Na B) H2 C) O2 D) Ca E) Li

Table 20.1Half Reaction E°(V)F2 (g) + 2e- → 2F- (aq) +2.87Cl2 (g) + 2e- → 2Cl- (aq) +1.359Br2 (l) + 2e- → 2Br- (aq) +1.065O2 (g) + 4H+ (aq) + 4e- → 2H2O (l) +1.23Ag+ + e- → Ag (s) +0.799Fe3+ (aq) + e- → Fe2+ (aq) +0.771I2 (s) + 2e- → 2I- (aq) +0.536

Cu2+ + 2e- → Cu (s) +0.342H+ + 2e- → H2 (g) 0

Pb2+ + 2e- → Pb (s) -0.126Ni2+ + 2e- → Ni (s) -0.28Li+ + e- → Li (s) -3.05

-21) Using Table 20.1, which substance can oxidize I (aq) to I2 (s) ?

A) Cu2+ (aq) B) Br- (aq) C) Ag (s) D) Br2 (l) E) Ni2+ (aq)


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Table 20.2Half-reaction E° (V)Cr3+ (aq) + 3e- → Cr (s) -0.74Fe2+ (aq) + 2e- → Fe (s) -0.440Fe3+ (aq) + e- → Fe2+ (s) +0.771Sn4+ (aq) + 2e- → Sn2+ (aq) +0.154

22) Which of the following reactions will occur spontaneously as written?

A) 3Sn4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq)

B) 3Fe2+ (aq) → Fe (s) + 2Fe3+ (aq)

C) Sn4+ (aq) + Fe3+ (aq) → Sn2+ (aq) + Fe2+ (aq)

D) Sn4+ (aq) + Fe2+ (aq) → Sn2+ (aq) + Fe (s)

E) 3Fe (s) + 2Cr3+ (aq) → 2Cr (s) + 3Fe2+ (aq)

23) Consider an electrochemical cell based on the reaction:2H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g)

Which of the following actions would change the measured cell potential?

A) increasing the [Sn2+] in the anode compartmentB) increasing the pressure of hydrogen gas in the cathode compartmentC) lowering the pH in the cathode compartmentD) increasing the pH in the cathode compartmentE) Any of the above will change the measure cell potential.

24) Consider an electrochemical cell based on the reaction:

2H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g)Which of the following actions would not change the measured cell potential?A) lowering the pH in the cathode compartmentB) increasing the pressure of hydrogen gas in the cathode compartmentC) addition of more tin metal to the anode compartmentD) increasing the tin (II) ion concentration in the anode compartmentE) Any of the above will change the measured cell potential.

25) Cathodic protection of a metal pipe against corrosion usually entailsA) attaching an active metal to make the pipe the anode in an electrochemical cell.B) coating the pipe with another metal whose standard reduction potential is less negative than that ofthe pipe.

C) attaching a dry cell to reduce any metal ions which might be formed.D) coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so hard tooxidize).

E) attaching an active metal to make the pipe the cathode in an electrochemical cell.


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26) One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell __________.A) electrons flow toward the anodeB) a nonspontaneous reaction is forced to occurC) O2 gas is produced at the cathode

D) oxidation occurs at the cathodeE) an electric current is produced by a chemical reaction

27) The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V:

Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)

With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.66 V. The concentration of H+ in the cathodecompartment is __________ M.

A) 2.0 × 10-2

B) 1.0 × 10-12C) 4.9 × 101

D) 4.2 × 10-4E) 1.4 × 10-1

28) A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is

AgCl (s) + e- → Ag (s) + Cl- (aq) E° = +0.222 V

The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M, respectively. The cellemf is __________ V.A) 0.232 B) 0.118 C) 22.2 D) 0.212 E) 0.00222

29) The standard emf for the cell using the overall cell reaction below is +2.20 V:

2Al (s) + 3I2 (s) → 2Al3+ (aq) + 6I- (aq)

The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [I-] = 0.15 M is ________ V.A) 2.39 B) 2.20 C) 2.23 D) 2.30 E) 2.10

30) The town of Natrium, West Virginia, derives its name from the sodium produced in the electrolysis ofmolten sodium chloride (NaCl) mined from ancient salt deposits. The number of kilowatt-hours ofelectricity required to produce 4.60 kg of metallic sodium from the electrolysis of molten NaCl(s) is__________ when the applied emf is 4.50 V.A) 0.0241 B) 24.1 C) 12.1 D) 0.0414 E) 48.3

2 Al (s) + Fe2O3 (s) Al2O3 (s) + 2 Fe (s) Which species undergoes reduction?


(A) Al (B) Al3+

(C) Fe (D) Fe3+

31. Given the reaction

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2. Which energy transformation occurs when an electrolytic cell is in operation?

Mg (s) + 2 AgNO3 (aq) Mg(NO3)2 (aq) + 2 Ag (s)

Which type of reaction is a REDOX reaction?

Given the reduction reaction for this cell:

Cu2+ (aq) + 2 e- Cu (s)

This reduction occurs at

(2) reduction (4) condensation

33. Given the reaction

34. Which equation shows conservation of both mass and charge?

cell. 35. The diagram below shows a key being plated with copper in an electrolytic

36. What is conserved during a chemical reaction?

37. Which type of reaction occurs when nonmetal atoms become negative nonmetal ions? oxidation (3) substitution


3 (A) chemical energy electrical energy (B) electrical energy chemical energy (C) light energy heat energy (D) light energy chemical energy

(A) single replacement (C) synthesis (B) double replacement (D) decomposition

(B) Cu + 2 Ag+ Cu2+ + Ag(C) Zn + Cr3+ Zn2+ + Cr (D) Ni + Pb2+ Ni2+ + Pb

(A) Cl2 + Br- Cl- + Br2

(A) A, which is the anode (B) A, which is the cathode(C) B, which is the anode (D) B, which is the cathode

(A) mass, only (B) charge, only (C) both mass and charge (D) neither mass nor charge

(1)

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Zn (s) + 2 HCl (aq) ZnCl2 (aq) + H2

Which statement correctly describes what occurs when this reaction takes place in a closed system?

2 Al + 3 Cu2+ 2 Al3+ + 3 Cu The reduction half reaction is

When the switch is closed, the electrons will flow from

38. Given the reaction:

39. A voltaic (Galvanic) cell differs from an electrolytic cell in that in a voltaic cell

41. How many electrons must be removed from elemental hydrogen (H2) to produce two

43. Given the equation:

44. A diagram of a electrochemical cell and an equation are shown below.


(A) Atoms of Zn (s) lose electrons and are oxidized(B) Atoms of Zn (s) lose electrons and are reduced. (C) There is a net loss of mass. (D) There is a net gain of mass.

(A) energy is produced when the reaction occurs (B) energy is required for the reaction to occur(C) both oxidation and reduction occur (D) neither oxidation nor reduction occur

40. What is the purpose of the salt bridge in a voltaic cell? (A) It blocks the flow of electrons (B) It blocks the flow of positive and negative ions. (C) It is a path for the flow of electrons. (D) It is a path for the flow of positive and negative ions.

moles of hydrogen ions (H+) in an aqueous solution (6.02 x 1023 electrons per 1 mole)? (A) 6.02 x 1023 (B) 12.04 x 1023 (C) 3.01 x 1023 (D) none of the above

42. Which statement is true for any electrochemical cell? (A) Oxidation occurs at the anode, only. (B) Reduction occurs at the anode, only. (C) Oxidation occurs at both the anode and cathode. (D) Reduction occurs at both anode and cathode.

(A) Al Al3+ + 3 e- (C) Al + 3 e- Al3+ (B) Cu2+ + 2 e- Cu (D) Cu2+ Cu + 2 e-

(A) the Pb (s) to the Cu (s) (B) the Cu (s) to the Pb (s)(C) the Pb2+ (aq) to the Pb (s) (D) the Cu2+ (aq) to the Cu (s)

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Which species undergoes reduction?

C (s) + H2O (g) CO (g) + H2 (g)

Mg (s) + 2 H+ (aq) + 2 Cl- (aq) --> Mg2+ (aq) + 2 Cl- (aq) + H2 (g) Which species undergoes oxidation?

(2) H+ (aq) (3) Cl- (aq) (4) H2 (g)

45. When a neutral atom undergoes oxidation, the atom’s oxidation state

46. Given the equation:

47. Given:

49. What is the oxidation number of chromium in K2Cr2O7?

-? 50. What is the oxidation number of manganese in MnO4

52. When 3.11 x 1024 Cr2O72– ion reduced in Cr3+, then how many ferrous (Fe2+) ionoxidised in ferric

(Fe3+) ion ?

51. How many electrons required to add for the reduction of one mole of MnO4

53. Theoretically, how many moles of iodide (I–) ion oxidized into iodate (IO3–) in using the no of

for the reduction of 24 moles of MnO4–


(A) decreases as it gains electrons(B) decreases as it loses electrons(C) increases as it gains electrons(D) increases as it loses electrons

(1) Mg (s)

48. Which particles are gained and lost during a redox reaction?

(A) electrons (C) neutrons (B) protons (D) positrons

(A) 12+ (C) 3+ (D) 6+

(A) C (s) (B) H+ (C) C2+ (D) H2 (g)

(A) -1 (B) 4- (C) 5+ (D) 7+

– in Mn2+ ?

(A) 1.8066 x 1024 (B) 3.011 x 1024 (C) 6.022 x 1024 (D) 1.2044 x 1024

(A) 1.8066 x 1024 (B) 1.2044 x 1024 (C) 6.022 x 1025 (D) 1.8066 x 1025

electrons required ion into Mn2+ ion ?

(A) 30 (B) 60 (C) 40 (D) 20

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56. What is in CH3COOCH3 respectively ?

58. What are the values of b, d and f in the balanced state of the following reaction?Reaction : aMnO4

–+bAs2O3+ cH2O ® dMn2++eASO4

59. In the balanced state of reaction, aBr2 + bOH– + CH2O ® dBrO4– + eHBr (basic medium),

if c=9, then what will be the change in oxidation no. (change

60. What will be the chage in the oxidation no. (change in no. of electrons) inbalanced eqation givenbelow ? Reaction : 2S + bHNO3 ® CH2SO4 + dNO (acidic medium)

61. What will be the chage in the oxidation no. (change in no. of electrons), if no. of e– = 10 inbalanced eqation given below ? Reaction : aP4 + bNO3

– + cH+ ® dPO43– + eNO2 + fH2O

(acidic medium)

the ratio of value of band c in the balanced equation given below ?

Reaction: aP4 + bNO3– + CH+ ® dPO4

which substance is oxidizes ? (mention it respectively)63. In the reaction, R – CHO + 2cuO ® R – COOH + Cu2O which substance is oxidising agent?And

or formalehydeacetaldehyde, acetone respectively ?

54. What is the oxidation no. of underlined C in HCHO, CH3CHO, CH3COOCH3

the oxidation no. of underlined C


(A) 0, +1, +2 (B) 0, +1, +3 (C) +1, 0, +3 (D) 0, +2, +155.

What is the oxidation no. of underlined C in HCHO, CH3CHO, CH3COOCH3 or methanol,acetic acid and methyl acetate respectively ?

(A) +2, +3, +3 (B) –2, +3, +3 (C) +2, +3, +4 (D) –2, +3, +4

(A) –3, +3, –3 (B) –3, +3, –2 (C) +3, +3, +3 (D) –2, +3, –2

57.In which of the following compound, oxidation no of all C atoms are same ?

(A) ethane (B) cyclohexane (C) benzene (D) given three compounds

3–+fH+(PH<7)

(A) 4, 5, 18 (B) 4, 10, 9 (C) 5, 4, 18 (D) 5, 4, 9

in no. of electrons).

(A) 21 (B) 7 (C) 14 (D) 9

(A) 6 (B) 3 (C) 12 (D) 9

(A) 20 (B) 10 (C) 5 (D) 15

62. What is

3– + eNO2 + fH2O (acidic medium)

(A) 5 : 2 (B) 10 : 3 (C) 2 : 5 (D) 1 : 1

(A) CuO, R–COOH (B) R–CHO, CuO (C) CuO, R–CHO (D) Cu2O, R–CHO

64. In which of the following reaction, H2O2 acts as oxidizing agent ?

(A) HOCl + H2O2 ® H3O+ + Cl– + O2 (B) I2 + H2O2 + 2OH– ® 2I– + 2H2O + O2

(C) PbS + 4H2O2 ® PbSO4 + 4H2O (D) In given all three.

65. In which of the following reaction, H2O2 as reducing agent ?

A) HNO2 + H2O ® HNO3 + H2O

(B) 2KMnO4 + 2H2O2 ® 2MnO2 + 2KOH + 2H2O + 3O2

(C) H2SO3 + H2O2 ® H2SO4 + H2O

(D) 2Fe2+ + H+ + H2O2 ® 2Fe3+ + H+ + H2O

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67. Which of the following is a no. of sulphur of H2SO3,H2S2O3, H2S2O7, H2S2O8or sulphurus acid, thio sulphuric acid, oleum, dithianic acid is arranged inascending

charge relateswith the reactiontheoretically ?

´ ´ ´ ´ 105 C

69. In the sample of ironoxide, the no. of Fe2+ ion is 90% and no. of is 10% then what is the molecularformula ?

would be the change in

+ bH2O + CO2® dH3PO4 +CO2,oxidation no. of oxygen decreases30,

73. Zn rod is dipped in a 1.5 litre aqueous solution of 0.1 M CuSO4 ;then choose the correct alternatefor given statements bassed on theoretical calculations. ( Atomic weight of Zn = 65gram – mole–1, Cu = 63.5 gram – mole–1) T= correct statement and

rod decreases, then 13 gm Zn metals in the solution

72. In a balanced equation, aP(S) then c–e=—

71. The oxidation

– then what coulomb of electric 68. When 0.25 mole I– oxidised in IO3

correct ascending order, when oxidation

2– + fNO + gH2O then what will bethe change in oxidation no. and the value of b

bNO3– cH+ ® 12Cu2+ + eSO474. In balanced equation, aCu2S +

1022 atoms of Cu deposited then concentration of Zn2+ ions in the solutionbecomes 0.04 M

´

1024.

(iv) when 3.6132

´and Zn2+ becomes equal in the solutoion then no. of Zn2+ ions in the

solution is 4.5165

0.08 M.

(iii) when molarity of Cu2+

gram Zn metal dissolve in the solution, then concentration of Cu2+ ion is (ii) 1.95


66. Which of the following is a redox reaction ?

(A) As2O3 + 3H2S ® As2S3 + 3H2O (B) 2NH3 + H2O + CO2 ® (NH4)2CO3

(C) CaO +3C ® CO + CaC2 (D) Be(OH)2 + 2HCl® BeCl2 + 2H2O

order ?

(A) H2SO3 < H2S2O3 < H2S2O7 < H2S2O6 (B) H2SO3 < H2S2O3 < H2S2O6 < H2S2O7

(C) H2S2O3 < H2SO3 < H2S2O7 < H2S2O6 (D) H2S2O3 < H2SO3 < H2S2O6 < H2S2O7

(A) 5.79 105 C (B) 4.82500 105 C (C) 2.895 105 C (D) 1.4475

(A) Fe0.905O (B) Fe0.952O (C) Fe0.825O (D) Fe0.857O70. In a

balanced equation, aLiH + bH2O2 ® CLi2O + dH2O (acidic medium), if d=6 then, whatno. of electrons and the value of a, b & c respectively

(A) 8, 4, 4, 2 (B) 4, 2, 2, 1 (C)4, 2, 1, 2 (D) 4, 4, 4, 2

no. of sulphur in Al2(SO4)3 is

(A) +8 (B) +7 (C) +5 (D) +6

(A) 3 (B) 1 (C) 2 (D) 4

F = false statement.

(i) 0.3 gram wt. of Zn

(A) TTTF (B) FFFT (C) TTFT (D) FFTT

and g respectively ?

(A) 30, 10, 8 (B) 121, 20, 16 (C) 24, 10, 8 (D) 60, 20, 16

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75.1 2

2+ +(c ) (C )Mg |Mg P Ag |Ag which of the following Nernst equation is correct for the given

electrochemical cell ?

2+°

+ 2

RT [Mg ]E cell = Ecell - .ln

2F [Ag ](b)

12+ 2

°+

RT [Mg ]E cell = Ecell - .ln

F [Ag ]

(c) 2+

°+

RT [Mg ]E cell=Ecell- .ln

2F [Ag ](d)

+ 2°

2+

RT [Ag ]E cell = Ecell - .ln

2F [Mg ]

76. For an electro chemical cell, 1

2+ 2+(C ) (0.5m)Zn| Zn || Cu |Cu , at constant temperature, reducing the

concentrations of both the solutions, then value of cell potential increases, then, what would bethe value of C1 ?

77.°

2+

E Cu = -0.34 volt

Cuand

° 2+

+

E Cu = +0.16 volt

Cu, then the value of

°

+

E Cu

Cu is ___.

H°+

(a)(1bar)

(P =11)2Pt|H |H half cell °25 C temperature ?

79. For an electrochemical cell, 2

2+ -(C1) (C ) 2(l)Mg|Mg ||Br |Br |Pt , what wiil be thechange in cell

potential, when conc of solution of cathode increase at constant

E cell=Eo cell

which of the following is thecorrect descending order of their strength of reducing agent

given all three statements are wrong.

vessel of of D2+ can be stored in the

vessel of in the

of A2+ can be stored

81. Standard oxidation potential of half cells of A/A2+, B/B2+, C/C2+ and D/D2+ are inincreasing order, then which of the following

80. Aqueous solution of salt of metal B is stored in a vesselof metal A and aqueous solution of soltof metal c can be storedin the vessel of metal B, then,


(a)

(A) 0.7 M (B) 0.5 M (C) 0.4 M (D) None of these

(A) –0.12v (B) –0.48v (C) +0.48v (D) –0.52v

78.What will be the oxidation potential of

(A) 0.177v (B) 0.649v (C) 0.282v (D) 0.616v

temperature ?

(A) increases (B) decreases (C) No change occurs(D)

A, B and c ?

(A) A > B > C (B) A > C > B (C) C > B > A (D) C > A > B

statement is correct ?

(A) solution of salt in the vessel of metal B.

(B) solution of salt of D2+ can’t be stored metal C.

(C) solution of salt metal B.

(D)

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82. For which of the following compound, a graph of mular conductivity and (molarity)1/2 is obtainedstraight line ?

having molten NaCl, CaCl2 and AlCl3 solutions are connected in series and sameelectricity is passed then, which of the following ratio of moles of metal obtained at cathode iscorrect ?

6:3:2

84. Eored for Fe/Fe2+ and Fe2+/Fe3+ half cells are –0.44volt and +0.77volt respectively then what willbe the value of Eoox

85. 5 faraday electric charge is passed during electrolysis of molten cacl2 solution, then what moles ofCa obtained at cathode experimentally ?

passed through electrolytic cells containing aqueous solutions ofCuSO4, AgNO3 and NiSO4, then what would be prportion of moles of metal obtained at differentcathodes respectively ?

1:2:1

87. What would be the change in PH of the solution, when electrolysis of aqueous solution ofCuSO4

is carried out

88. Which of the following formula is true to calculate the molar conductivity in conventionalsymbols ?

m=C×A

^ (b) 1000×G×A

=mC×l

^ (c)1000×G×l

=mC×A

^ (d) 1000×C×l

=mR×A

^

89. 2 -1KCl- NaCl=23.4Mho (cm) mole° °^ ^ and 2 -1NaSr- NaCl=1.8Mho -(cm) -mole

°°^ ^ then,

which of the following is the correct order of molar conductivity at intimite dilution in an ascendingpattern?

gram Ag is deposited at cathode. If 6 90. In an experiment of electroplating, 4 ampere electric current is passed for 2 minutes. Hence, m

ampere current is passed for 40 second, then what amountAg is deposited at


(A) CsCl (B) NH4OH (C) HCOOH (D) given all three

83. Electrolytic cells

(A) 1:2:3 (B) 3:2:1 (C) 6:2:3 (D)

for Fe/Fe3+ half cell ?

(A) 0.037v (B) 0.33v (C) –0.33v (D) –o.11v

(A) 2.5 mole (B) less then 2.5 mole (C) more then 2.5 mole (D) 5 mole

86. When same electric charge is

(A) 2:1:2 (B) 2:2:1 (C) 1:1:2 (D)

in presence of inert electrodes ?

(A) PH increasses (B) PH decreases (C) no change in PH (D) can’t be predicted

1000×R×l(a)

(A) NaCl < KCl < NaBr < KBr (C) NaCl < NaBr < KCl < KBr

(B) KBr < NaCl < NaBr < KCl (D) KCl < NaCl < NaBr < KBr

cathode ?

(A) 2m (B) 4m (C) m/2 (D) m/4

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nernst equation to

potential of Cu/Cu2+ half cell ?

(a) ° 2+ ° 2+ 2+RT

E Cu|Cu =E Cu|Cu - ×ln[Cu ]2F

(b) ° 2+ ° 2+ 2+RT

E Cu|Cu =E Cu|Cu + ×ln[Cu ]2F

(c) ° 2+ 2+ 2+RT

E Cu|Cu =E Cu|Cu + ×ln[Cu ]2F

(d) ° 2+ 2+

2+

RT 1E Cu|Cu -E Cu|Cu = ×ln×

2F [Cu ]

92. The values of for m°^ AA2B, X3Y2 and A3Y are 2.4, 1.5 and 1.8 respectively. Then what will be the

value of m°

93. What amount of electric charge required for the reduction of 1 mole Cr2O72– into Cr3+

95. In an shows Ecell

96. For the electrochemical cell, 2

2+ +(C )Mg|Mg (0.04m)||Ag |Ag ; Ecell = Eocell, then what will

be the value of C2

97. In an electrochemical cell, 1

2+ 2+(C ) (0.4m)Fe|Fe ||Cu |Cu , at constant temperature, concentration of both

the solutions increases equally, then cell potential increases. Thus which od the following will

be the value of C1 ?

electrochemical cell for which of the following alternative

does the potential of

and Ered of cathode become equal

the half

is in equilibrium, then

conductance at 98. Which of the following possesses maximum equivalent

1 bar pressure, oxidation potential of hydrogen half cell is 0.118volt, then what would be the POH of the

charge obtained from the cell?cell is

–50k.cal then what coulomb electric 99. The potential of a cell is 2.0 volt. change in free energy (SG) occur for the reaction of


91. Which of the following is correct form of the

determine the oxidation

^ for XB ?

(A) 1.7 mho – (cm)2 – mole–1 (B) 8.1 mho – (cm)2 – mole–1

(C) 2.1 mho – (cm)2 – mole–1 (D) 0.7 mho – (cm)2 – mole–1

theoretically ?

(A) 6 (B) 3 (C) 1 (D) 4

94. What the electrochemical cell become zero ?

(A) Eox of anode

(B) Eored of anode and Eored of cathode become equal

(C) Ered of anode and Ered of cathode become equal

(D) Concentration of both the half cell become same

= Eocell ?

(A) k = 1, then... (B) cell reaction

(C) concentration of both cells become equal, then (D) None of these

?

(A) 0.04 M (B) 0.02 M (C) 0.2 M (D) 0.0016M

(A) 0.8 M (B) 0.1 M (C) 0.4 M (D) None of these

infinite dilution?

(A) K+(aq) (B) Na+

(aq) (C) Cs+(aq)(aq) (D) Rb+

(A) 1.08 c (B) 104600 c (C) 25000 c (D) 0.26 c

100. A+ 25° c temperature and solution?

(A) 2 (B) 3 (C) 5 (D) 12

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1) B2)A3) A4) B

7) B8) E9) B10) A11) D12) A

5) D6) C

15) C16) E17) A18) C19) A20) C21) D22) A23) E

26) B27) A

24) C25) E

Answer31.d 32.b 33.a 34.d 35.b 36.c 37. b38.a 39.a 40. d 41.b 42.a43.b 44.a 45.d 46.b 47.a 48.a 49.d 50.d

13) A14) A

28) B29) D30) B

JEE-UNIT-81 c 99 bd2 b 51 b 100 d3 a 52 d4 a 53 d5 a 54 a6 b 55 b7 d 56 b8 d 57 d9 c 58 c10 c 59 a11 a 60 c12 a 61 a13 b 62 b14 b 63 c15 d 64 c16 a 65 b17 c 66 c18 d 67 d19 d 68 d20 c 69 b21 a 70 a22 c 71 d23 c 72 a24 a 73 c25 c 74 d26 c 75 b27 d 76 c28 b 77 d29 c 78 a30 a 79 b31 c 80 c32 c 81 c33 d 82 a34 a 83 d35 c 84 a36 a 85 b37 d 86 d38 c 87 b39 a 88 c40 b 89 b41 b 90 c42 b 91 c43 c 92 a44 c 93 a45 a 94 c46 b 95 d47 c 96 c48 b 97 a49 a 98 c


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chapter 20 quiz - ibiokaare.com · _____ kj/mol. pb (s) + 2h+ (aq ... how many grams of cus are...

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