JEE MAINS - VOL - VI REDOX REACTIONS
2) molar conductance
ELECTROLYTIC CONDUCTANCE
3) specific conductance
4) specific resistance
19. The best conductor of electricity is a 1M 30. If the specific conductance and conductance
solution of of a solution are same, then its cell constant
1) Boric acid 2) Acetic acid is equal to:
3) H2SO4 4) Phosphoric acid 1) 1 2) 0 3) 10 4) 100
20. Which of the following aqueous solutions will 31. A solution of concentration ‘C’ g equiv/litre
conduct an electric current quite well? has a specific resistance R. The equivalent
1) Sugar 2) Glycerol conductance of the solution is
3) Pure water 4) HCl 1000 C
1) 2)
21. Pure water does not conduct electricity RC R
because it is R 1000R
1) Neutral 3) 4)
C C
2) Readily decomposed 32. Which of the following is correct for the
3) Almost unionised solution of C2 H 5COOH upon dilution
4) Completely ionised
regarding current carrying species?
22. In aqueous solution, strong electrolytes
ionize and yield 1) The number in 1 cm 3 as well as in total volume
1) Ions 2) Electrons increases
3) Acids 4) Oxides 2) The number in 1 cm 3 decreases whereas that
23. Which of the following is a poor conductor in the total volume remains constant
of electricity 3) The number in 1 cm 3 decreases but that in the
1) CH3COONa 2) C2H5OH total volume increases
3) NaCl 4) KOH 4) The number in 1 cm3 as well as in total volume
decreases.
24. Arrhenius theory is applicable only to 33. If x is the specific resistance of the solution
1) weak electrolyte 2) Strong electrolyte and N is the normality of the solution. Then
3) both 1 & 2 4) non electrolyte
equivalent conductivity of the solution is
25. Which of the following does not conduct
current in aqueous solution given by
1) KNO3 2) CH3COOH 1000x 1000 1000N Nx
3) CH3 OH 4) NaOH 1) 2) 3) 4)
N Nx x 1000
26. Which of the following solid is an electronic 34. Which of the following solutions has the
conductor
highest equivalent conductance?
1) NaCl 2) Diamond
3) CuS 4) KCl 1) 0.5 M NaCl 2) 0.05 M NaCl
27. The units of conductivity of solution are 3) 0.005 M NaCl 4) 0.02 M NaCl
35. Debye-Huckel-Onsager equation is
1) ohm1 2) ohms
3) ohm 1cm 1 4) ohm1eq 1 represented as c 0 b c . ‘b’ is
28. The unit of cell constant is 82.4 8.20 105
1) (DT)1/2 ^0
1) ohm1 2) ohm - cm (DT)3/2
3) cm 1 4) ohm 1cm2 eq 1
82.4 8.20 105
29. The cell constant is the product of resistance 2) (DT)1/2 ^0
and (DT)1/2
1) conductance
Bapuji
NISHITH Multimedia
SPSS IndiaTolahunse
PU College, (Pvt.. Ltd., 99
,REDOX REACTIONS JEE MAINS - VOL - VI
82.4 8.20 105 PHENOMENON OF ELECTROLYSIS
3) (DT)1/2
(DT)1/2
41. Electrolysis of salt solution is due to the
8.24 8.20 10 5 formation of
4) (DT)1/2 (DT)1/2 ^ 0 1) Electron 2) Ions
3) Oxides 4) Acids
36. What happens at infinite dilution in a given
42. The reactions taking place at anode and
solution ?
cathode of a cell respectively are
1) The degree of dissociation is unity for weak
1) Reduction, oxidation
electrolytes
2) Oxidation, reduction
2) The electrolyte is 100% ionised
3) Hydrolysis, oxidation
3) All inter ionic attractions disappear
4) Reduction, hydrolysis
4) All the three
43. Electrode at which electrons flow into the
37. The relationship m 0m B C will not electrolyte is
hold good for the electrolyte? 1) Anode 2) Cathode
3) Both anode & cathode 4) +ve electrode
1) HCl 2) KCl 3) BaCl2 4) HCN
44. In an electrolytic cell current flows from
1) Cathode to anode in outer circuit
KOHLRAUSCH’S LAW AND 2) anode to cathode outside the cell
APPLICATIONS 3) cathode to anode inside the cell
4) Current does not flow
38. The Kohlrausch law is related to 45. During electrolysis electrons flow from
1) Conductance of ions at infinite dilution 1) cations to cathode 2) anode to anions
2) Independent migration of ions 3) cathode to anode 4) anions to anode
3) Both 1 and 2 46. The cathode of an electrolysis and a reducing
4) Neither 1 and 2 agent are similar because both
39. The expression showing the relationship 1) are metals 2) supply electrons
between equivalent conductance and molar 3) remove electrons 4) Absorb electrons
conductance is (z = Total positive (or) 47. The cathode reaction in electrolysis of dilute
negative charge per formula unit of sulphuric acid with Platinum electrode is
electrolyte) 1) Oxidation
1) m Z eq 2) eq Z m 2) Reduction
3) Both oxidation and reduction
eq
3) m 2
4) m eq 4) Neutralization
Z 48. Schematic diagram of an electrolytic-cell is:
40. The equation representing Kohlrausch law
from the following is ( V+ = No. of cations,
V– = No. of anions
100K
1) m C V V
2) 0m v 0 v .0
m
1000K
3) eq C V
V 4) 0m c a
eq
100 Bapuji SPSS PU College, Tolahunse
,JEE MAINS - VOL - VI REDOX REACTIONS
3) gram molecular mass
4) Gram atomic ions
54. The electric charge for electrode deposition
of 1gm. Equivalent of a substance is
1) 96,500 coulombs
1) 2) 2) One ampere per sec
3) One ampere for one hour
4) Charge in faradays
55. The number of faradays required to liberate
1 mole of any element indicates
1) weight of the element.
2) conductance of the electrolyte
3) 3) charge on the ion of the element
4) isotopic number
56. 6.24 x 1019 electrons is equal approximately
4) None is correct presentation to
1) 10 coulombs 2) 96500 coulombs
FARADAY’S LAWS AND APPLICATIONS 3) one electron volt 4) 0.1F
49. Faraday’s laws of electrolysis are related ELECTROCHEMICAL SERIES
to the & EMF
1) molecular mass of the electrolyte
2) Equivalent weight of the cation /anion 57. The metal which cannot liberate H2 gas from
3) Atomic weight of the electrolyte hydrochloric acid
4) Atomic number of the cation/anion 1) Zn 2) Cu 3) Mg 4) Al
50. The unit of electrochemical equivalent is 58. For which of the following SOP and SRP are
1) Gram 2) Gram / Ampere equal
3) Gram / Coulomb 4) Coulomb / Gram 1. SHE 2. Mg Electrode
51. When 1 amp of current is passed through 3. Ni electrode 4. copper electrode
an electrolyte for one second, the mass 59. The electrode potential measures the
1) tendency of the electrode to gain or lose
deposited is equal to
electrons
1) 1 mole of hydrogen
2) electron affinity of elements
2) 1 gram equivalent of hydrogen
3) difference in the ionization potential of
3) 1 electro–chemical equivalent
electrode and metal ion
4) 1 gram of any substance
4) heat of combustion
52. On electrolysis 1 mole Al atoms will be 60. The potential across the metal and the
deposited by aqueous solution of its ions of unit activity
1) 1 mole of electrons at 298K is known as
2) 2 moles of electrons 1) Electrode potential
3) 3 moles of electrons 2) Standard electrode potential
4) 6 moles of electrons 3) Formal electrode potential
53. When the same quantity of electricity is 4) Oxidation potential
passed through the solution of different 61. Which one of the following metal will not
electrolytes in series, the amount of product reduce H2O?
obtained are proportional to their
1) Ca 2) Fe
1) Atomic weights
3) Cu 4) Li
2) Chemical Equivalent
Bapuji
NISHITH Multimedia
SPSS IndiaTolahunse
PU College, (Pvt.. Ltd., 101
, REDOX REACTIONS JEE MAINS - VOL - VI
62. Arrange the following in the order of their n
2.303 RT M
decreasing electrode potentials: Mg, K, 0
2) E E log
Ba,Ca nF M
1) K,Ba,Ca,Mg 2) Ba,Ca,K,Mg n
2.303 RT M
3) Ca,Mg,K,Ba 4) Mg,Ca,Ba,K 0
3) E E log
63. For the cell reaction to be spontaneous the nF M
EMF of the cell should be 2.303 RT
1) negative 4) E E 0 log Mn
nF
2) positive
68. The potential of a single electrode depends
3) zero
upon
4) some times positive and some times –ve
1) the nature of the electrode
64. The EMF of a galvanic cell is determined
by using a 2) temperature
1) Voltmeter 3) concentration of the ion with respect to which
2) Spectrometer it is reversible
3) Coulometer 4) all the above
4) Ammeter 69. The relationship between standard reduction
65. Cathodic standard reduction potential potential of a cell and equilibrium constant
minus anodic standard reduction potential is shown by
is equal to n 0.059
1) Faraday 2) coulomb 1) E0cell logK c 2) E0cell logK c
0.059 n
3) cell potential 4) Ampere
logK c
66. Consider following sets 3) E0cell 0.059nlogK c 4) E0cell
n
70. The relationship between free energy and
electrode potential is
1) G nFE 2) G nFE
nFE H
3) G 4) G
R nFE
ELECTROCHEMCIAL CELLS
71. Which of the following energy changes
Blue colour solution changes to colourless occur in galvanic cell?
(or fades) in: 1) Electrical energy Chemical Energy
1) I, II, III 2) I, II 2) Chemical Energy Electrical Energy
3) II, III 4) I, III 3) Chemical Energy Internal Energy
4) Internal Energy Electrical Energy
NERNST EQUATION 72. In a galvanic cell electron flow will be from
1) Negative electrode to positive electrode
67. The Nernst equation giving dependence of 2) Positive electrode to negative electrode
electrode potential on concentration is 3) There will be no flow of electrons
2.303 RT M 4) Cathode to anode in the external circuit
0
1) E E nF
log
Mn 73. In a galvanic cell, the reactions taking place
in the anodic half cell and the cathodic half
cell will be
102 Bapuji SPSS PU College, Tolahunse
2) molar conductance
ELECTROLYTIC CONDUCTANCE
3) specific conductance
4) specific resistance
19. The best conductor of electricity is a 1M 30. If the specific conductance and conductance
solution of of a solution are same, then its cell constant
1) Boric acid 2) Acetic acid is equal to:
3) H2SO4 4) Phosphoric acid 1) 1 2) 0 3) 10 4) 100
20. Which of the following aqueous solutions will 31. A solution of concentration ‘C’ g equiv/litre
conduct an electric current quite well? has a specific resistance R. The equivalent
1) Sugar 2) Glycerol conductance of the solution is
3) Pure water 4) HCl 1000 C
1) 2)
21. Pure water does not conduct electricity RC R
because it is R 1000R
1) Neutral 3) 4)
C C
2) Readily decomposed 32. Which of the following is correct for the
3) Almost unionised solution of C2 H 5COOH upon dilution
4) Completely ionised
regarding current carrying species?
22. In aqueous solution, strong electrolytes
ionize and yield 1) The number in 1 cm 3 as well as in total volume
1) Ions 2) Electrons increases
3) Acids 4) Oxides 2) The number in 1 cm 3 decreases whereas that
23. Which of the following is a poor conductor in the total volume remains constant
of electricity 3) The number in 1 cm 3 decreases but that in the
1) CH3COONa 2) C2H5OH total volume increases
3) NaCl 4) KOH 4) The number in 1 cm3 as well as in total volume
decreases.
24. Arrhenius theory is applicable only to 33. If x is the specific resistance of the solution
1) weak electrolyte 2) Strong electrolyte and N is the normality of the solution. Then
3) both 1 & 2 4) non electrolyte
equivalent conductivity of the solution is
25. Which of the following does not conduct
current in aqueous solution given by
1) KNO3 2) CH3COOH 1000x 1000 1000N Nx
3) CH3 OH 4) NaOH 1) 2) 3) 4)
N Nx x 1000
26. Which of the following solid is an electronic 34. Which of the following solutions has the
conductor
highest equivalent conductance?
1) NaCl 2) Diamond
3) CuS 4) KCl 1) 0.5 M NaCl 2) 0.05 M NaCl
27. The units of conductivity of solution are 3) 0.005 M NaCl 4) 0.02 M NaCl
35. Debye-Huckel-Onsager equation is
1) ohm1 2) ohms
3) ohm 1cm 1 4) ohm1eq 1 represented as c 0 b c . ‘b’ is
28. The unit of cell constant is 82.4 8.20 105
1) (DT)1/2 ^0
1) ohm1 2) ohm - cm (DT)3/2
3) cm 1 4) ohm 1cm2 eq 1
82.4 8.20 105
29. The cell constant is the product of resistance 2) (DT)1/2 ^0
and (DT)1/2
1) conductance
Bapuji
NISHITH Multimedia
SPSS IndiaTolahunse
PU College, (Pvt.. Ltd., 99
,REDOX REACTIONS JEE MAINS - VOL - VI
82.4 8.20 105 PHENOMENON OF ELECTROLYSIS
3) (DT)1/2
(DT)1/2
41. Electrolysis of salt solution is due to the
8.24 8.20 10 5 formation of
4) (DT)1/2 (DT)1/2 ^ 0 1) Electron 2) Ions
3) Oxides 4) Acids
36. What happens at infinite dilution in a given
42. The reactions taking place at anode and
solution ?
cathode of a cell respectively are
1) The degree of dissociation is unity for weak
1) Reduction, oxidation
electrolytes
2) Oxidation, reduction
2) The electrolyte is 100% ionised
3) Hydrolysis, oxidation
3) All inter ionic attractions disappear
4) Reduction, hydrolysis
4) All the three
43. Electrode at which electrons flow into the
37. The relationship m 0m B C will not electrolyte is
hold good for the electrolyte? 1) Anode 2) Cathode
3) Both anode & cathode 4) +ve electrode
1) HCl 2) KCl 3) BaCl2 4) HCN
44. In an electrolytic cell current flows from
1) Cathode to anode in outer circuit
KOHLRAUSCH’S LAW AND 2) anode to cathode outside the cell
APPLICATIONS 3) cathode to anode inside the cell
4) Current does not flow
38. The Kohlrausch law is related to 45. During electrolysis electrons flow from
1) Conductance of ions at infinite dilution 1) cations to cathode 2) anode to anions
2) Independent migration of ions 3) cathode to anode 4) anions to anode
3) Both 1 and 2 46. The cathode of an electrolysis and a reducing
4) Neither 1 and 2 agent are similar because both
39. The expression showing the relationship 1) are metals 2) supply electrons
between equivalent conductance and molar 3) remove electrons 4) Absorb electrons
conductance is (z = Total positive (or) 47. The cathode reaction in electrolysis of dilute
negative charge per formula unit of sulphuric acid with Platinum electrode is
electrolyte) 1) Oxidation
1) m Z eq 2) eq Z m 2) Reduction
3) Both oxidation and reduction
eq
3) m 2
4) m eq 4) Neutralization
Z 48. Schematic diagram of an electrolytic-cell is:
40. The equation representing Kohlrausch law
from the following is ( V+ = No. of cations,
V– = No. of anions
100K
1) m C V V
2) 0m v 0 v .0
m
1000K
3) eq C V
V 4) 0m c a
eq
100 Bapuji SPSS PU College, Tolahunse
,JEE MAINS - VOL - VI REDOX REACTIONS
3) gram molecular mass
4) Gram atomic ions
54. The electric charge for electrode deposition
of 1gm. Equivalent of a substance is
1) 96,500 coulombs
1) 2) 2) One ampere per sec
3) One ampere for one hour
4) Charge in faradays
55. The number of faradays required to liberate
1 mole of any element indicates
1) weight of the element.
2) conductance of the electrolyte
3) 3) charge on the ion of the element
4) isotopic number
56. 6.24 x 1019 electrons is equal approximately
4) None is correct presentation to
1) 10 coulombs 2) 96500 coulombs
FARADAY’S LAWS AND APPLICATIONS 3) one electron volt 4) 0.1F
49. Faraday’s laws of electrolysis are related ELECTROCHEMICAL SERIES
to the & EMF
1) molecular mass of the electrolyte
2) Equivalent weight of the cation /anion 57. The metal which cannot liberate H2 gas from
3) Atomic weight of the electrolyte hydrochloric acid
4) Atomic number of the cation/anion 1) Zn 2) Cu 3) Mg 4) Al
50. The unit of electrochemical equivalent is 58. For which of the following SOP and SRP are
1) Gram 2) Gram / Ampere equal
3) Gram / Coulomb 4) Coulomb / Gram 1. SHE 2. Mg Electrode
51. When 1 amp of current is passed through 3. Ni electrode 4. copper electrode
an electrolyte for one second, the mass 59. The electrode potential measures the
1) tendency of the electrode to gain or lose
deposited is equal to
electrons
1) 1 mole of hydrogen
2) electron affinity of elements
2) 1 gram equivalent of hydrogen
3) difference in the ionization potential of
3) 1 electro–chemical equivalent
electrode and metal ion
4) 1 gram of any substance
4) heat of combustion
52. On electrolysis 1 mole Al atoms will be 60. The potential across the metal and the
deposited by aqueous solution of its ions of unit activity
1) 1 mole of electrons at 298K is known as
2) 2 moles of electrons 1) Electrode potential
3) 3 moles of electrons 2) Standard electrode potential
4) 6 moles of electrons 3) Formal electrode potential
53. When the same quantity of electricity is 4) Oxidation potential
passed through the solution of different 61. Which one of the following metal will not
electrolytes in series, the amount of product reduce H2O?
obtained are proportional to their
1) Ca 2) Fe
1) Atomic weights
3) Cu 4) Li
2) Chemical Equivalent
Bapuji
NISHITH Multimedia
SPSS IndiaTolahunse
PU College, (Pvt.. Ltd., 101
, REDOX REACTIONS JEE MAINS - VOL - VI
62. Arrange the following in the order of their n
2.303 RT M
decreasing electrode potentials: Mg, K, 0
2) E E log
Ba,Ca nF M
1) K,Ba,Ca,Mg 2) Ba,Ca,K,Mg n
2.303 RT M
3) Ca,Mg,K,Ba 4) Mg,Ca,Ba,K 0
3) E E log
63. For the cell reaction to be spontaneous the nF M
EMF of the cell should be 2.303 RT
1) negative 4) E E 0 log Mn
nF
2) positive
68. The potential of a single electrode depends
3) zero
upon
4) some times positive and some times –ve
1) the nature of the electrode
64. The EMF of a galvanic cell is determined
by using a 2) temperature
1) Voltmeter 3) concentration of the ion with respect to which
2) Spectrometer it is reversible
3) Coulometer 4) all the above
4) Ammeter 69. The relationship between standard reduction
65. Cathodic standard reduction potential potential of a cell and equilibrium constant
minus anodic standard reduction potential is shown by
is equal to n 0.059
1) Faraday 2) coulomb 1) E0cell logK c 2) E0cell logK c
0.059 n
3) cell potential 4) Ampere
logK c
66. Consider following sets 3) E0cell 0.059nlogK c 4) E0cell
n
70. The relationship between free energy and
electrode potential is
1) G nFE 2) G nFE
nFE H
3) G 4) G
R nFE
ELECTROCHEMCIAL CELLS
71. Which of the following energy changes
Blue colour solution changes to colourless occur in galvanic cell?
(or fades) in: 1) Electrical energy Chemical Energy
1) I, II, III 2) I, II 2) Chemical Energy Electrical Energy
3) II, III 4) I, III 3) Chemical Energy Internal Energy
4) Internal Energy Electrical Energy
NERNST EQUATION 72. In a galvanic cell electron flow will be from
1) Negative electrode to positive electrode
67. The Nernst equation giving dependence of 2) Positive electrode to negative electrode
electrode potential on concentration is 3) There will be no flow of electrons
2.303 RT M 4) Cathode to anode in the external circuit
0
1) E E nF
log
Mn 73. In a galvanic cell, the reactions taking place
in the anodic half cell and the cathodic half
cell will be
102 Bapuji SPSS PU College, Tolahunse
