JEE Questions for Chemistry Electrochemistry Quiz 4 - MCQExams.com

Molar conductance of electrolytic solution Ʌm is
  • ∝ l
  • ∝ (1/A)
  • ∝ (1/C)
  • ∝ (√C)
The molar conductivities Ʌo NaOAc and Ʌo HCl at infinite dilution in water at 25oC are 91.0 and 426.2 S cm2/mol respectively. To calculate ɅoHOAc, the additional value required is
  • ɅoH2O
  • ɅoKCl
  • ɅoNaOH
  • ɅoNaCl
Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100 Ω. The conductivity of this solution is 1.29 Sm-1 . Resistance of the same cell when filled with 0.2 M of the same solution is 520Ω. The molar conductivity of 0.02 M solution of the electrolyte will be
  • 124 × 10-4 S m2 mol-1
  • 1240 × 10-4 S m2 mol-1
  • 1.24 × 10-4 S m2 mol-1
  • 12.4 × 10-4 S m2 mol-1
Which one of the following has the highest molar conductivity ?
  • Diaminedichloroplatinum (II)
  • Tetraaminedichlorocobalt (III) chloride
  • Potassium hexacyanoferrate (II)
  • Hexaaquochromium (III) bromide
  • Pentacarbonyl iron (0)
Ionisation depends upon
  • pressure
  • volume
  • dilution
  • None of these
The highest electrical conductivity of the following aqueous solutions is of
  • 0.1 M difluoroacetic acid
  • 0.1M fluoroacetic acid
  • 0.1 M chloroacetic acid
  • 0.1 M acetic acid
The quantity of electricity required to libreate 112 cm3 of hydrogen at STP from acidified water is
  • 965 Coulombs
  • 1 Faraday
  • 0.1 Faraday
  • 96500 Coulombs
A silver cup is plated with silver by passing 965 C of electricity. The amount of Ag deposited is
  • 107.89 g
  • 9.89 g
  • 1.0002 g
  • 1.08 g
During the electrolysis of molten NaCl solution, 230 g of sodium metal is deposited on the cathode, then how many moles of chlorine will be obtained at anode?
  • 10.0
  • 5.0
  • 35.5
  • 17.0
By passing 9.65 A current for 16 min 40 s, the volume of O2, liberated at STP will be
  • 280 mL
  • 560 mL
  • 1120 mL
  • 2240 mL
Which substance is obtained in the solution on electrolysis of aqueous CuSO2 solution using graphite electrodes?
  • H2O
  • H2SO4
  • Na2SO4
  • Cu(OH)2
Use of electrolysis is not done in
  • production of Na
  • production of water
  • purification of metals
  • production of KOH
Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 mA current. The time required to liberate 0.01 mole of H2 gas at the cathode is (1F = 96500 C mol-1 )
  • 9.65 × 104 s
  • 19.3 × 104 s
  • 28.95 × 104 s
  • 38.6 × 104 s
When same quantity of electricity is passed through aqueous AgNO3 and H2 SO4 solutions connected in series, 5.04 × 10-2 g of H2 is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen =1.008, silver = 108)
  • 54
  • 0.54
  • 5.4
  • 10.8
The amount of electricity required to produce one mole of copper from copper sulphate solution will be
  • 1 F
  • 2.33 F
  • 2 F
  • 1.33 F
A current of 12 A is passed through an electrolytic cell containing aqueous NiSO4 solution. Both Ni and H2 gas are formed at the cathode. The current efficiency is 60%. What is the mass of nickel deposited on the cathode per hour?
  • 7.883 g
  • 3.941 g
  • 5.91 g
  • 2.645 g
The cathodic reaction of a dry cell is represented by
2MnO2 (s) + Zn2+ + 2e‒ → ZnMn2 O4 (s)
If, there arc 8 g of MnO2, in the cathodic compartment then the time for which the dry cell will continue to give a current of 2 mA is
  • 25.675 day
  • 51.35 day
  • 12.8 day
  • 6.423 day
In acidic medium MnO-4 is converted to Mn2+. The quantity of electricity in Faraday required to reduce 0.5 mole of MnO-4 to Mn2+ would be
  • 2.5
  • 5
  • 1
  • 0.5
During electrolysis of water the volume of O2 liberated is 2.24 dm3. The volume of hydrogen liberated, under same conditions will be
  • 2.24 dm3
  • 1.12 dm3
  • 4.48 dm3
  • 0.56 dm3
What is the time (in sec) required for depositing all the silver present in 125 mL of 1 M AgNO3 solution by passing a current of 241.25 A ? (1F = 96500 C)
  • 10
  • 50
  • 1000
  • 100
Assertion (A) A current of 96.5 A is passed into aqueous AgNO3 solution for 100 s. The weight of silver deposited is 10.8 g (Atomic weight of Ag =
Reason (R) The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
  • Both A and R are correct and R is the correct explanation of A
  • Both A and R are correct but R is not the correct explanation of A
  • A is correct but R is incorrect
  • A is incorrect but Reason is correct
The laws of electrolysis were proposed by
  • Kohlrausch
  • Faraday
  • Haber
  • Bergius
What is the quantity of electricity (in Coulombs) required to deposit all the silver from 250 mL of 1 MAgNO3 solution ?
  • 2412.5
  • 24125
  • 4825.0
  • 48250
Which of the following is not correct ?
  • Aqueous solution of NaCl is an electrolyte
  • The units of electrochemical equivalent are g-coulomb
  • In the Nernst equation, n represents the number of electrons transferred in the electrode reaction
  • Standard reduction potential of hydrogen electrode is zero volt.
Given below are the half- cell reactions
Mn2+ + 2e‒ → Mn; Eo = ‒ 1.18e V
2(Mn3+ + e‒ → Mn2+) Eo = + 1.51e V
The Eo for 3 Mn2+ → Mn + 2Mn3+ will be
  • ‒2.69V, the reaction will not occur
  • ‒2.69 V, the reaction will occur
  • ‒0.33 V, the reaction will not occur
  • ‒0.33 V, the reaction will occur
What is the cell potential (standard emf, E°) for the reaction below ?
[E°(Fe2/(aq)Fe) = 0.44 V and E°(O2(g)/H2O/OH ‒ ) = + 0.4V]
2Fe (s) + O2 (g) + 2H2O (l) ⇌ 2Fe2+ (aq) + 4OH ‒ (aq)

  • Chemistry-Electrochemistry-3284.png
  • 2)
    Chemistry-Electrochemistry-3285.png

  • Chemistry-Electrochemistry-3286.png

  • Chemistry-Electrochemistry-3287.png

Chemistry-Electrochemistry-3289.png
  • 2
  • 3
  • 5
  • 4
Zinc is used to reduce iron because
  • Ered of Zn < Ered of Fe
  • Eoxi of Zn < Eoxide of Fe
  • Eoxi of Zn = Eoxide of Fe
  • Zinc is cheaper than iron

Chemistry-Electrochemistry-3291.png
  • Ag2O
  • Al2O3
  • MgO
  • Na2O

Chemistry-Electrochemistry-3292.png
  • Cl
  • Cr3+
  • Mn2+

  • Chemistry-Electrochemistry-3293.png
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