JEE Questions for Chemistry Electrochemistry Quiz 1 - MCQExams.com

The specific conductance (κ) of an electrolyte of 0.1 N concentration is related to equivalent conductance (Ʌ) by the following formula
  • Ʌ = κ
  • Ʌ = 10κ
  • Ʌ = 100 κ
  • Ʌ = 10000 κ
The resistance of 1N solution of acetic acid is 250Ω, when measured in a cell having a cell constant of 1.15 cm-1. The equivalent conduction (in ohm-1 cm2 equiv-1) of 1N acetic acid is
  • 2.3
  • 4.6
  • 9.2
  • 18.4
The one which decreases with dilution is
  • molar conductance
  • conductance
  • specific conductance
  • equivalent conductance
Given the limiting molar conductivity as
˄0m (HCl) = 425.9Ω-1 cm2 mol-1
˄0m (NaCl) = 126.4Ω-1 cm2 mol-1
˄0m (CH3 COONa) = 91Ω-1 cm2 mol-1
The molar conductivity, at infinite dilution, of acetic acid (in Ω-1 cm2 mol-1
) will be
  • 481.5
  • 390.5
  • 299.5
  • 516.9
The molar conductivities of KCl, NaCl and KNO3 are 152, 128 and 111 S cm2mo1-1 respectively. What is the molar conductivity of NaNO3 ?
  • 101 S cm2 mol-1
  • 87 S cm2 mol-1
  • -101 S cm2 mol-1
  • -391 S cm2 mol-1
Which one of the following solutions will have highest conductivity?
  • 0.01 M CH3 COOH
  • 0.1 M NaCl
  • 0.1 M KNO3
  • 0.1 M HCl
Which of the following electrolytic solutions has the least specific conductance?
  • 0.02 N
  • 0.2 N
  • 2 N
  • 0.002 N
Which of the following does not conduct electricity?
  • Fused NaCl
  • Solid NaCl
  • Brine solution
  • Copper
For strong electrolytes the plot of molar conductance vs√C is
  • parabolic
  • linear
  • sinusoidal
  • circular
The units of equivalent conductance, are
  • Ω cm2 equiv-1
  • Ω cm2 equiv
  • Ω-1 cm2 equiv-1
  • Ω cm2 equiv
Pure water does not conduct electricity because it is
  • basic
  • almost not ionised
  • decomposed easily
  • acidic
What is the effect of dilution on the equivalent conductance of strong electrolyte ?
  • Decreases on dilution
  • Remains unchanged
  • Increases on dilution
  • None of these
Given. l/a = 0.5 cm-1, R = 50 ohm, N = 1.0 . The equivalent conductance of the electrolytic cell is
  • 10 Ω-1 cm2 g equiv-1
  • 20 Ω-1 cm2 g equiv-1
  • 300 Ω-1 cm2 g equiv-1
  • 100 Ω-1 cm2 g equiv-1
Impure copper containing Fe, Au, Ag as impurities is electrolytically refined. A current of 140 A for 482.5s and decreased the mass of the anode by 22.26 g and increased the mass of cathode by 22.011 g percentage of iron in impure copper is (given molar mass Fe = 55.5 g / mol; molar mass of Cu = 63.54 g/mol)
  • 0.95
  • 0.85
  • 0.97
  • 0.9
When 9.65 C of elecricity is passed through a solution of silver nitrate (atomic mass of Ag =108 g mol-1) , the amount of silver deposited is
  • 16.2 mg
  • 21.2 mg
  • 10.8 mg
  • 6.4 mg
Silver is monovalent and has an atomic mass of 108. Copper is divalent and has an atomic mass of 63.6. The same electric current is passed, for the same length of time through a silver coulometer and a copper coulometer. If 27.0 g of silver is deposited, then the corresponding amount of copper deposited is
  • 63.60 g
  • 31.80 g
  • 15.90 g
  • 7.95 g
  • 4.00 g
The approximate time duration in hours to electroplate 30g of calcium from molten calcium chloride using a current of 5 A is (At. mass of Ca =
  • 80
  • 10
  • 16
  • 8
Read the following statetnent and predict the corresponding law? 'At infinite dilution when dissociation is complete, each ion makes a definite contribution towards total equivalent conductance of the electrolyte irrespective of the nature of the ion.
  • Ostwald's-dilution law
  • Kohlrausch's law
  • Nernst equation
  • Ohm's law
9.65 C of electric current is passed through fused anhydrous MgCl2 . The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of Grignard reagent obtained is
  • 5 × 10-4
  • 1 × 10-4
  • 5 × 10-5
  • 1 × 10-5
What will be pH of aqueous solution of electrolyte in electrolytic cell during electrolysis of CuSO4 (aq) between graphite electrodes?
  • pH = 14.0
  • pH > 7.0
  • pH < 7.0
  • pH = 7.0
Two different electrolytic cells filled with molten Cu (NO3 )2 and molten Al(NO3 )3 respectively are connected in series. When electricity is passed 2.7 g Al is deposited on electrode. Calculate the weight of Cu deposited on cathode.
(Cu = 63.5, Al = 27.0 g mol-1)
  • 190.5 g
  • 9.525 g
  • 63.5 g
  • 31.75 g
Give the products available on the cathode and the anode respectively during the electrolysis of an aqueous solution of MgSO4 between inert electrodes.
  • H2 (g) and O2 (g)
  • O2 (g) and H2 (g)
  • O2 (g) and Mg (s)
  • O2 (g) and SO2 (g)
A solution of CuSO4 is electrolysed for 10 min with a current of 1.5 A. What is the mass of copper deposited at the cathode?
  • 2.096 g
  • 0.296 g
  • 3.029 g
  • 2.096 g
In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under STP condition. The current to be passed is
  • 1.93 A
  • 9.65 A
  • 19.3 A
  • 0.965 A
If 'F' is Faraday and 'N' is Avogadro number, then charge of electron can be expressed as
  • F × N
  • F/N
  • N/F
  • F2 N
The amount of substance deposited by the passage of lA of current for 1 s is equal to
  • equivalent mass
  • molecular mass
  • electrochemical equivalent
  • specific equivalent
When a quantity of electricity is passed through CuSO4 solution, 0.16 g of copper gets deposited. If the same quantity of electricity is passed through acidulated water, then the volume of H2 liberated at STP will be (given, atomic weight of Cu =
  • 4.0 cm3
  • 56 cm3
  • 604 cm3
  • 8.0 cm3
How long (in hours) must a current of 5.0 A be maintained to electroplate 60 g of calcium from molten CaCl2?
  • 27 h
  • 8.3 h
  • 11 h
  • 16 h
The amount of silver deposited on passing 2 F of electricity through aqueous solution of AgNO3 is
  • 54 g
  • 108 g
  • 216 g
  • 324 g
When during electrolysis of a solution of AgNO3, 9650C of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be
  • 1.08 g
  • 10.8 g
  • 21.6 g
  • 108 g
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