Class 12 Chemistry Chapter 2 Electrochemistry MCQ

Class 12 Chemistry Chapter 2 Electrochemistry MCQ: On this page we have given Class 12 Chemistry Chapter 2 Electrochemistry Multiple Choice (MCQ) Question and Answer for students of CBSE board. Students will very much helpful for this question and answer.

Electrochemistry Class 12 MCQ with Answers:

(1) The study of production of electricity from energy released during spontaneous chemical reactions and use of electrical energy to bring about non-spontaneous chemical transformations, is known as –

(a) Solution

(b) Electrochemistry

(c) Daniell cell

(d) Galvanic Cell

Ans: (b) Electrochemistry

(2) Which type of cell converts the chemical energy liberated during the redox reaction?

(a) Galvanic cell

(b) Voltaic cell

(c) Daniell Cell

(d) Electrolytic cell

Ans: (c) Daniell Cell

(3) To electrical energy and has an electrical potential equal to 1.1 V when concentration of zn²⁺ and Cu²⁺ ions is unity such a device is called a –

(a) Daniell cell

(b) Electrolytic cell

(b) Galvanic cell

(d) Both a and b

Ans: (b) Galvanic cell

(4) Galvanic cell is also known as –

(a) Electrolytic cell

(b) Voltaic cell

(c) Daniell cell

(d) Chemistry cell

Ans: (b) Voltaic cell

(5) What is the value of Ecxt. When no flow of electrons or current and no chemical reaction.

(a) Eext = 1.1V

(b) Eext > 1.1V

(c) Eext < 1.1V

(d) Eext = 1.2V

Ans: (a) Eext = 1.1V

(6) What is the value of Eext, when electrons flow from Cu to Zn and current flows from Zn to Cu and Zinc is deposited at the zinc electron and copper dissolves at copper electrode.

(a) Eext = 1.1V

(b) Eext > 1.1V

(c) Ecxt < 1.1V

(d) Ecxt = 1.2V

Ans: (b) Eext > 1.1V

(7) What is the value of Eext, when electrons flow from Zn rod to Cu rod hence current flows from Cu to Zn and Zn dissolves at anode and copper deposits at cathode.

(a) Ecxt = 1.1V

(b) Eext = 2.5V

(c) Ecxt <1.1V

(d) Ecxt > 1.1V

Ans: (c) Ecxt <1.1V

(8) The reduction half reaction occurs on the copper electrode while the oxidation half reaction occurs on the Zinc electrode. This two portions of the cell are also called as –

(a) Half-cells

(b) Redox couples

(c) Gibbs energy

(d) Both a and b

Ans: (d) Both a and b

(9) The copper electrode may be called –

(a) Reduction half-cell

(b) Oxidation half-cell

(c) Redox half-cell

(d) Both a and b

Ans: (a) Reduction half-cell

(10) The Zinc electrode may be called –

(a) Reduction half cell

(b) Oxidation half cell

(c) Redox Half cell

(d) Both a and b

Ans: (b) Oxidation half cell

(11) A potential difference develops between the electrode and the electrolyte which is called –

(a) Electrode potential

(b) Standard electrode potential

(c) Anode

(d) Cathode

Ans: (a) Electrode potential

(12) When the concentrations of all the species involved in a half-cell is unity then the electrode potential is known as –

(a) Electrode potential

(b) Anode

(c) Cathode

(d) Standard electrode potential

Ans: (d) Standard electrode potential

(13) In Galvanic cell the half cell in which oxidation takes place is called –

(a) Anode

(b) Cathode

(c) Redox couples

(d) Gibbs Energy

Ans: (a) Anode

(14) In galvanic cell, other half cell in which reduction takes place is called –

(a) Gibbs energy

(b) Redox couples

(c) Anode

(d) Cathode

Ans: (d) Cathode

(15) The potential difference between the two electrodes of a galvanic cell is called –

(a) Electrode potential

(b) Cell potential

(c) Gibbs energy

(d) Half-cells

Ans: (b) Cell potential

(16) What does cell potential measure?

(a) Mole

(b) Volts

(c) Centimeters

(d) Grams

Ans: (b) Volts

(17) The cell potential is the difference between the electrode potentials of the cathode and anode, it is called as the –

(a) Standard electrode potential

(b) Electrode potential

(c) Cell electromotive force

(d) Potential energy

Ans: (c) Cell electromotive force

(18) H⁺ (aq) + e^– à?

(a) 1H⁺

(b) H₂

(c) 1/2 H₂

(d) H

Ans: (c) 1/2 H₂

(19) What is the emf value of following reaction:

F₂(g) + 2e^– à 2f^–

(a) 1.87V

(b) 0.34V

(c) -0.44V

(d) 2.87V

Ans: (d) 2.87V

(20) H₂O₂ + 2H⁺ + 2e^– à 2H₂ O

What is the emf value of this reaction?

(a) 2.87V

(b) -0.74V

(c) 0.97

(d) 1.78V

Ans: (d) 1.78V

(21) What is emf value of following reaction?

Li + e^– à Li (s)

(a) -2.93V

(b) -3.05V

(c) 2.71V

(d) -3.58V

Ans: (b) -3.05V

(22) What is the emf value of reaction –K⁺+e^– à k (s)?

(a) -3.05V

(b) -2.87V

(c) -2.93V

(d) -2.36V

Ans: -2.93V

(23) What is the emf value of following reaction:

Pb²⁺ + 2e^– à Pb (s)

(a) -0.14V

(b) 0.00V

(c) -0.13V

(d) -0.44V

Ans: (c) -0.13V

(24) 2H₂O + 2e^– à H₂(g) + 2OH^– (aq) ‘

What is the emf value of this reaction?

(a) – 0.83V

(b) -0.44V

(c) -0.39V

(d) -4.07V

Ans: (a) – 0.83V

(25) Na⁺+ e^– à Na (s)

(a) -2.44V

(b) -2.71V

(c) -2.34V

(d) -4.05V

Ans: (b) -2.71V

(26) What is the emf value of following reaction?

m_rO₂(s) + 4H⁺ + 2e⁺ à m_r²⁺+ 2H₂O

(a) 1.23V

(b) 0.00V

(c) -0.13V

(d) 0.80V

Ans: (a) 1.23V

(27) What is the emf value of following reaction?

m_nO4^– + 8H⁺ + 5e^– à m_n²⁺ + 4H₂O

(a) 1.58V

(b) 1.51V

(c) 1.78V

(d) 1.81V

Ans: (b) 1.51V

(28) Cr₂O_>^2- + 14H⁺ + 6e^– à 2Cr3 + 7H2O

What is emf value for this reaction?

(a) 1.36V

(b) 1.33V

(c) 0.97V

(d) 0.80V

Ans: (b) 1.33V

(29) H₂O₂ + 2H⁺ + 2e^– à 2H₂O

What is the emf value for this reaction?

(a) 1.81V

(b) 2.87V

(c) 1.78V

(d) 1.33V

Ans: (c) 1.78V

(30) What is the emf value for following reaction?

2H⁺ + 2e^– à H₂ (g)

(a) 0.10V

(b) -0.44V

(c) 0.00V

(d) 0.34V

Ans: (c) 0.00V

(31) Following are the which type of equation:

E (cell) = E° (Cell) – RT/nF InQ

(a) Daniell cell equation

(b) Cell potential equation

(c) Nernst equation

(d) Galvanic cell equation

Ans: (c) Nernst equation

(32) Respect the cell in which the following reaction takes place (s) + 2 Ag⁺ (0.0001M) à Mg²⁺ (0.130M) + 2Ag (s) calculate its E (cell) if E° (cell) = 3.17V

(a) 2.96V

(b) 3.12V

(c) 4.45V

(d) 0.45V

Ans: (a) 2.96V

(33) Calculate the equilibirium constant of the reaction:

Cu(s) + 2Ag⁺ (aq) à Cu²⁺(aq) + 2Ag (s)

E°(cell) = 0.40V

(a) 1.41 × 10^-6

(b) 3.92 × 10¹⁵

(c) 3.49 × 10^-15

(d) 2.42 × 10⁶

Ans: 3.92 × 10¹⁵

(34) What is the equation for gibbs energy of the reaction –

(a) △rG = nFE (Cell)

(b) △rG = -nFE (Cell)

(c) △rG = FE (Cell)

(d) △rG  -FE (Cell)

Ans: (b) △rG = -nFE (Cell)

(35) The standard electrode potential for Daniell cell is 1.1V calculate the standard Gibbs energy for the reaction:

Zn(s) + Cu²⁺(aq) à Zn²⁺ (aq) + Cu (s)   

(a) -212.27 KJmol^-1

(b) -214.28 KJmol^-1

(c) 47.29 KJmol^-1

(d) 329.21  KJmol^-1

Ans: (a) -212.27 KJmol^-1

(36) Calculate the emf of the cell in which the following reaction takes place:

Ni (s) + 2Ag⁺ (0.002M) à Ni²⁺ (0.160M) + 2Ag (s)

Given that E° (cell) = 1.05V

(a) 1.24V

(b) 0.91V

(c) 2.94V

(d) 4.49V

Ans: (b) 0.91V

(37) The cell in which the following reactions occurs: 2fe³⁺(aq.) + 2I^–(aq.) à 2Fe²⁺(aq.) + I₂(s) has E°(cell) = 0.236V at 295K. Calculate the standard Gibbs Energy.

(a) 0.114

(b) 4.445

(c) 5.423

(d) 0.345

Ans: (a) 0.114

(38) The cell in which the following reaction occurs: 2fe³⁺(aq.) + 2I^–(aq.) à 2Fe²⁺(aq.) + I₂(s) has E°(cell) = 0.236V at 295K. Calculate the equillibirium constant of the cell reaction.

(a) 3.45×10^-4molL^-1

(b) 4.55×10^-3molL^-1

(c) 3.67 × 10^-4 molL^-1

(d) 4.79 × 10^-3 molL^-1

Ans: (c) 3.67 × 10^-4 molL^-1

(39) P is called as ….. (e-rho)

(a) Resistivity

(b) Conductance

(c) Constant

(d) Conductivity

Ans: (a) Resistivity

(40) R is called as –

(a) Resistivity

(b) Conductance

(c) Conductivity

(d) Temperature

Ans: (b) Conductance

(41) What is the unit to measure electrical resistance?

(a) Volt

(b) Mol

(c) Ohm

(d) Ohm Metre

Ans: (c) Ohm

(42) What is the SI Unit of electrical resistance?

(a) Kgm²

(b) Kgm²/S³A²

(c) Sm²

(d) Sm^-1

Ans: (b) Kgm²/S³A²

(43) The electrical resistance is directly proportional to –

(a) Area

(b) Length

(c) Diameter

(d) Radius

Ans: (b) Length

(44) The electrical resistance of any object is inversely proportional to –

(a) Length

(b) Diameter

(c) Radius

(d) Area

Ans: (d) Area

(45) 1 Ω m is equal to –

(a) 0.01 cm

(b) 0.01 Ω cm

(c) 100 Ω cm

(d) 0.1 Ω cm

Ans: (d) 0.1 Ω cm

(46) 1 Ω cm =?

(a) 0.01 Ω cm

(b) 0.01 Ω m

(c) 100 Ω m

(d) 0.1 Ω m

Ans: (b) 0.01 Ω m

(47) What is the SI unit of conductance?

(a) Ohm

(b) Voltage

(c) Mole

(d) Siemens

Ans: (d) Siemens.

(48) Siemens is also equal to –

(a) Ohm^-1

(b) Ohm^-1m

(c) Ohm^-1 Cm

(d) Ohm

Ans: (a) Ohm^-1

(49) Inverse of resistivity called as –

(a) Conductance

(b) Resistivity

(c) Conductivity

(d) Resistance

Ans: (c) Conductivity

(50) What is the SI unit of conductivity?

(a) Sm^-1

(b) S cm^-2

(c) Sm²

(d) S cm²

Ans: (a) Sm^-1

(51) What is the value conductivity of sodium conductors at 298.15K?

(a) 5.9 × 10³

(b) 2.1 × 10³

(c) 6.2 × 10³

(d) 1.2 × 10³

Ans: (b) 2.1 × 10³

(52) What is the value of conductivity of Gold conductors at 298.15K?

(a) 1.0 × 10³

(b) 5.1 × 10³

(c) 6.2 × 10³

(d) 4.5 × 10³

Ans: (d) 4.5 × 10³

(53) What is the value of conductivity of glass insulators at 298.15K?

(a) 1.0 × 10^-16

(b) 1.2 × 10^-16

(c) 4.5 × 10^-16

(d) 5.9 × 10^-16

Ans: (a) 1.0 × 10^-16

(54) What is the value of conductivity of pure water aqueous solution at 298.15K?

(a) 2.1 × 10^-5

(b) 2.5 × 10³

(c) 1.0 × 10^-18

(d) 3.5 × 10^-5

Ans: (d) 3.5 × 10^-5

(55) What is the value of conductivity of 0.1M HCL of aqueous solution at 298.15K?

(a) 2.14×10^-5

(b) 2.4×10³

(c) 3.91

(d) 1.0×10^-18

Ans: (c) 3.91

(56) What is the value of conductivity of 0.1M HAC of aqueous solution at 298.15K?

(a) 0.016

(b) 0.047

(c) 0.12

(d) 0.14

Ans: (b) 0.047

(57) What is the value of conductivity of 0.01 M Nacl aqueous solution at 298.15K?

(a) 0.016

(b) 0.047

(c) 0.12

(d) 0.91

Ans: (c) 0.12

(58) What is the value of conductivity of CuO semi conductor at 298.15K?

(a) 1×10^-7

(b) 1.5×10^-2

(c) 2.0

(d) 2.4×10³

Ans: (a) 1×10^-7

(59) What is the value of conductivity of Si semiconductor at 298.15K?

(a) 1×10^-7

(b) 2.0

(c) 1.5×10^-2

(d) 2.9

Ans: 1.5×10^– 

(60) Metals and their alloys have very large conductivity, are known as –

(a) Semiconductors

(b) Conductors

(c) Insulators

(d) Superconductors

Ans: (b) Conductors

(61) Substances like glass, ceramics etc having very low conductivity are known as –

(a) Semiconductors

(b) Insulators

(c) Conductors

(c) Superconductors

Ans: (b) Insulators

(62) Substances having conductivity between conductors and insulators are called as –

(a) Insulator

(b) Conductors

(c) Semiconductors

(d) Superconductors

Ans: (c) Semiconductors

(63) Electrical conductance through metals is called as –

(a) Metallic conductance

(b) Electronic conductance

(c) Metalloid Conductance

(d) Both a and b

Ans: (d) Both a and b

(64) The electronic conductance depends on –

(a) Nature and structure of metal

(b) Number of valence electron

(c) Temperature

(d) All of the above

Ans: (d) All of the above

(65) Who was awarded the Noble Prize in chemistry for the year 2000 for discovery of conducting polymer?

(a) Mac Diamid

(b) Heeger

(c) Shirakawa

(d) All of the above

Ans: (d) All of the above

(66) The conductance o electricity by ions present in the solutions is called –

(a) Electronic conductance

(b) Ionic conductance

(c) Electronic conductance

(d) Both a and b

Ans: (d) Both a and b

(67) Conductivity of electrolytic solutions depends on –

(a) The nature of electrolytic added

(b) Temperature

(c) Concentration of the electrolytic

(d) All of the above

Ans: (d) All of the above

(68) The quantity l/a is called as –

(a) Conductance

(b) Cell constant

(c) Resistance

(d) Conductivity

Ans: (b) Cell constant

(69) What is symbol denoted for cell constant?

(a) C*

(b) G*

(c) K

(d) G

Ans: (b) G*

(70) What is the conductivity in 5cm^-1 of KCl solutions at 298.15K of molarity = 1.000 molL^-1?

(a) 11.13

(b) 0.113

(c) 0.0129

(d) 1.29

Ans: (b) 0.113

(71) What is the conductivity in 5m^-1 of KCl solutions at 298.15K of molarity = 0.010 ——?

(a) 100.0

(b) 0.0129

(c) 10.00

(d) 1000

Ans: (c) 10.00

(72) What is the molar conductivity in Sm²mol^-1 of KCl solution at 298.15K of molarity – 0.100 mol-1 ?

(a) 111.3 × 10^-4

(b) 0.0129 ×10^-4

(c) 141.0 ×10^-4

(d) 129.0 ×10^-4

Ans: (d) 129.0 ×10^-4

(73) What is the molar conductivity in Scm²mol^-1 of KCl solution at 298 15K of Molarity  1000 mol m^-3? 

(a) 111.3

(b) 129.0

(c) 141.0

(d) 0.0129

Ans: (a) 111.3

 

(74) What is the symbol denoted for molar conductivity?

(a) Λ

(b) Λm

(c) Ω

(d) G*

Ans: (b) Λm

(75) What is the equation used for molar conductivity?

(a) Λm = G*/R

(b) Λm = K/C

(c) Λm = G*/C

(d) Λm = K/R

Ans: (b) Λm = K/C

(76) What is the unit used for Λm?

(a) Sm^-1

(b) mol m^-3

(c) sm² mol^-1

(d) Smol^-1

Ans: (c) sm² mol^-1

(77) Resistance of a conductivity cell filled with 0.1 molL^-1 KCl solutions is 100Ω. If the resistance of the same cell when filled with 0.02 molL^-1 KCl solution 520Ω. Calculate the conductivity of 0.02 molL^-1 KCl solution. Conductivity of 0.1 molL^-1 KCl solution is 1.29, S/m.

(a) 0.456×10^-2 Sm²

(b) 0.248×10^-2 Scm^-1

(c) 229.6×10^-6Sm^-1

(d) 45.6×10^-6Sm^-1

Ans: (b) 0.248×10^-2 Scm^-1

(78) The electrical resistance of a column 0.05 molL^-1 NaoH solution of diameter 1cm and length 50cm is 5.55×10³Ω calculate is resistivity?

(a) 87.135 Ωcm

(b) 229.6 Scm²mol^-1

(c) 47.124 Ω cm

(d) 22.445 Ω cm

Ans: (a) 87.135 Ωcm

(79) The electrical resistance of a column of 0.05 molL^-1 NaoH solution of diameter 1cm and length 50cm is 5.55 × 10³Ohm. Calculate its molar conductivity? (R = 87.135Ωcm)

(a) 2.245 Scm² mol^-1

(b) 2.224 Scm²mol^-1

(c) 229.6 Scm² mol^-1

(d) 0.113 Scm²mol^-1

Ans: (c) 229.6 Scm² mol^-1

(80) What is the limiting molar conductivity of H⁺ ion in water —– 298K?

(a) 50.1 Scm²mol^-1

(b) 119.0 Scm²mol^-1

(c) 349.6 Scm² mol^-1

(d) 73.5 Scm² mol^-1

Ans: (c) 349.6 Scm² mol^-1

(81) What is the limiting molar conducting of K⁺ ion in water at 298K?

(a) 50.1 Scm² mol^-1

(b) 73.5 Scm² mol^-1

(c) 106.0 Scm² mol^-1

(d) 119.0 Scm²mol⁷

Ans: (b) 73.5 Scm² mol^-1

(82) What is the limiting molar conductivity of ca²⁺ ion in water at 298K?

(a) 119.0 Scm² mol^-1

(b) 73.5 Scm² mol^-1

(c) 50.5 Scm² mol^-1

(d) 40.1 Scm² mol^-1

Ans: (a) 119.0 Scm² mol^-1

(83) What is the limiting molar conductivity of CH₃COO^– ion in water at 298K?

(a) 78.1 Scm² mol^-1

(b) 40.1 Scm² mol^-1

(c) 40.9 Scm² mol^-1

(d) 78.5 Scm² mol^-1

Ans: (c) 40.9 Scm² mol^-1

(84) What is the limiting molar conductivity of —- ion in water at 298K?

(a) 40.9 Scm²mol^-1

(b) 78.1 Scm²mol^-1

(c) 76.3 Scm²mol^-1

(d) 160.0 Scm² mol^-1

Ans: (d) 160.0 Scm² mol^-1

(85) What is the symbol denoted for limiting molar conductivity?

(a) G*

(b) Λm

(c) λ°

(d) λ°m

Ans: (c) λ°

(86) What is the unit of limiting molar conductivity?

(a) Scm²mol^-2

(b) Cm²mol^-1

(c) Scm²mol^-1

(d) Smol^-1

Ans: (c) Scm²mol^-1

(87) Calculate Λ°m for CaCl₂ from the data given below –

λCa²⁺ = 119.0 Scm² mol^– ; λCl^–  76.3 Scm² mol^-1

(a) 271.6 Scm² mol^-1

(b) 266 Scm² mol^-1

(c) 27.61 Scm²mol^-1

(d) 78.4 Scm²mol^-1

Ans: (a) 271.6 Scm² mol^–

(88) Calculate Λ°m for MgSO₄ from the data given below –

λ° mg²⁺ = 106.0 Scm² mol^-1 ; λ° —— = 160.0 Scm² mol^-1

(a) 271.6 Scm²mol^-1

(b) 27.61 Scm²mol^-1

(c) 266 Scm²mol^-1

(d) 78.46 Scm² mol^-1

Ans: (c) 266 Scm²mol^-1

(89) Λ°m for NaCl, HCl and NaAc are 126.4, 425.9 and 91.0 Scm²mol^-1 respectively calculate Λ° for HAC?

(a) 266 Scm² mol^-1

(b) 44.48 Scm²mol^-1

(c) 30.5 Scm² mol^-1

(d) 390.5 Scm² mol^-1

Ans: (d) 390.5 Scm² mol¹

(90) The Conductivity of 0.001028 molL^-1 acetic acid is 4.95×10^-5 S cm². Calculate —- dissociation constant if Λ°m for acetic acid is 390.5 S cm² mol¹.

(a) 48.15 Scm² mol^-1

(b) 1.78×10^-5molL^-1

(c) 2.44×10^-5molL^-1

(d) 4.55×10^-5 molL^-1

Ans: (b) 1.78×10^-5molL^-1

(91) The molar conductivity of 0.025 molL^-1 methanoic acid is 46.1 S cm² mol^-1. Calculate its degree of dissociation given λ°(H⁺) = 349.6 S cm² mol^-1 and λ° (HCOO^–) = -54.6 Scm²mol^-1

(a) – 0.223

(b) -0.114

(c) 5.654

(d) 4.225

Ans: (b) -0.114

(92) The molar conductivity of 0.025 molL^-1 methanoic acid is 46.1 S cm²mol^-1. Calculate its dissociation constant. Given λ° (H⁺) = 349.65 cm² mol^-1 and λ° (HCOO^–) = 54.6 S cm²mol^-1

(a) 3.67 × 10^-4 molL^-1

(b) 4.47 × 10^-4molL^-1

(c) 3.46 × 10^-4molL^-1

(d) 4.56 × 10^-4molL^-2

Ans: (a) 3.67 × 10^-4 molL^-1

(93) Who was firstly described the quantitative aspects of electrolysis?

(a) Henry

(b) Michael Faraday

(c) Kohlrausch

(d) Dalton

Ans: (b) Michael Faraday

(94) A solution of CuSO₄ is electrolysed for 10 minutes with a current of 1.5 ampheres. What is the mass of copper deposited at the cathode?

(a) 0.427g

(b) 0.2938g

(c) 2.432g

(d) 4.489g

Ans: (b) 0.2938g

(95) If a current of 0.5 ampere flows a through metallic wire for 2 hours then flow many electrons would flow through the wire?

(a) 4.45×10⁶ electrons

(b) 5.46×10²² no. of electrons

(c) 2.25×10²² no. of electrons

(d) 4.67×10⁶ no. of electrons

Ans: (c) 2.25×10²² no. of electrons

(96) Galvanic cells that are designed to convert the energy of combustion of fuels like hydrogen, methane, methanol etc. Directly into electrical energy are called as –

(a) Anode cells

(b) Cathode cells

(c) Fuel cells

(d) Memory cells

Ans: (c) Fuel cells

(97) 2 fe(s) + O₂(g) + 4H⁺ (aq.) à 2fe⁺(aq.) + 2H₂O (l)

E° (cell) =?

(a) 2.27V

(b) 1.23V

(c) 1.67V

(d) 0.44V

Ans: (c) 1.67V

Read: Coordination Compounds Class 12 MCQs