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11th Class Chemistry Chapter 10 MCQs with Answers

11th Class Chemistry Chapter 10 MCQs

Enhance your knowledge of Electrochemistry MCQs with topics like oxidation-reduction, electrochemical cells, and electrode potentials. These Chapter 10 quizzes are tailored for 11th Class Chemistry students aiming to excel.

Which of the following is a chemical change involving the transfer of electrons?
a) Evaporation
b) Sublimation
c) Oxidation-reduction
d) Dissolution

Answer
c) Oxidation-reduction

The electrode where reduction occurs is called the:
a) Anode
b) Cathode
c) Electrolyte
d) None of the above

Answer
b) Cathode

Which type of cell converts chemical energy into electrical energy spontaneously?
a) Electrolytic cell
b) Galvanic cell
c) Fuel cell
d) Voltaic cell

Answer
b) Galvanic cell

The electrode where oxidation occurs is called the:
a) Anode
b) Cathode
c) Electrolyte
d) None of the above

Answer
a) Anode

In a galvanic cell, electrons flow from the anode to the cathode through the:
a) Electrolyte
b) Salt bridge
c) External circuit
d) Cell membrane

Answer
c) External circuit

Which of the following is the standard reduction potential of hydrogen electrode?
a) 0.00 V
b) +1.00 V
c) -1.00 V
d) +0.34 V

Answer
a) 0.00 V

The standard reduction potential of any half-cell is measured with respect to the:
a) Anode
b) Cathode
c) Hydrogen electrode
d) Salt bridge

Answer
c) Hydrogen electrode

Which of the following represents the cell notation for a galvanic cell?
a) Anode | Cathode || Electrolyte
b) Cathode | Anode || Electrolyte
c) Electrolyte | Cathode || Anode
d) Anode || Cathode | Electrolyte

Answer
a) Anode | Cathode || Electrolyte

The flow of positive charge in an electrochemical cell occurs through the:
a) Anode
b) Cathode
c) Electrolyte
d) External circuit

Answer
d) External circuit

The movement of ions in the salt bridge is essential to maintain:
a) Charge neutrality
b) Electrode potential
c) Cell voltage
d) Electrolytic conductivity

Answer
a) Charge neutrality

The reduction potential of a species is a measure of its ability to:
a) Gain electrons
b) Lose electrons
c) Be oxidized
d) Be reduced

Answer
a) Gain electrons

Which of the following is a common application of electroplating?
a) Rust prevention
b) Cooking
c) Water purification
d) Generating electricity

Answer
a) Rust prevention

In the Nernst equation, E is the cell potential, E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, and n is the number of:
a) Electrons transferred
b) Protons transferred
c) Moles of solute
d) Moles of solvent

Answer
a) Electrons transferred

Which of the following statements is true for a spontaneous reaction?
a) ∆G > 0
b) ∆G = 0
c) ∆G < 0
d) ∆G is not defined

Answer
c) ∆G < 0

The electrolysis of water produces hydrogen gas at the:
a) Anode
b) Cathode
c) Both anode and cathode
d) None of the above

Answer
b) Cathode

The process of a metal being corroded by natural agents such as air and water is known as:
a) Electrolysis
b) Oxidation
c) Reduction
d) Rusting

Answer
d) Rusting

Which of the following is not a strong electrolyte?
a) Sodium chloride (NaCl)
b) Hydrochloric acid (HCl)
c) Ethanol (C2H5OH)
d) Sulfuric acid (H2SO4)

Answer
c) Ethanol (C2H5OH)

The electrochemical equivalent of a substance is defined as the amount of substance deposited or liberated at the electrode per unit:
a) Current
b) Time
c) Charge
d) Temperature

Answer
c) Charge

The Faraday constant (F) represents the charge of:
a) 1 mole of electrons
b) 1 mole of protons
c) 1 mole of ions
d) 1 mole of neutrons

Answer
a) 1 mole of electrons

Which of the following is used as a reference electrode in electrochemical measurements?
a) Calomel electrode
b) Copper electrode
c) Platinum electrode
d) Silver chloride electrode

Answer
a) Calomel electrode

A redox reaction is a combination of:
a) Oxidation and reduction reactions
b) Acid and base reactions
c) Double displacement reactions
d) Precipitation reactions

Answer
a) Oxidation and reduction reactions

Which of the following is the correct representation of the cell notation for a galvanic cell involving copper and zinc electrodes?
a) Cu | Zn || CuSO4 || ZnSO4
b) Cu | CuSO4 || ZnSO4 || Zn
c) Zn | ZnSO4 || CuSO4 || Cu
d) Zn | CuSO4 || ZnSO4 || Cu

Answer
c) Zn | ZnSO4 || CuSO4 || Cu

The quantity of electricity required to deposit one mole of any substance is called:
a) Faraday’s law
b) Faraday’s constant
c) Electrochemical equivalent
d) Electrolysis constant

Answer
c) Electrochemical equivalent

Electrolysis is commonly used for the extraction of which metal from its ore?
a) Gold
b) Iron
c) Copper
d) Silver

Answer
c) Copper

Which of the following is a non-spontaneous reaction?
a) ∆G > 0
b) ∆G = 0
c) ∆G < 0
d) ∆G is not defined

Answer
a) ∆G > 0

The process of using a sacrificial metal to protect another metal from corrosion is known as:
a) Electrolysis
b) Cathodic protection
c) Anodic protection
d) Galvanic cell

Answer
b) Cathodic protection

Which of the following is used as the anode in a lead-acid battery?
a) Lead dioxide (PbO2)
b) Sulfuric acid (H2SO4)
c) Lead (Pb)
d) Carbon

Answer
c) Lead (Pb)

The standard hydrogen electrode (SHE) is assigned a standard reduction potential of:
a) +0.34 V
b) -0.34 V
c) +1.00 V
d) 0.00 V

Answer
d) 0.00 V

Which of the following is an example of an inert electrode?
a) Copper electrode
b) Platinum electrode
c) Zinc electrode
d) Iron electrode

Answer
b) Platinum electrode

The oxidation half-reaction involves the:
a) Gain of electrons
b) Loss of electrons
c) Formation of anions
d) Formation of cations

Answer
b) Loss of electrons

Which of the following is a strong electrolyte?
a) Acetic acid (CH3COOH)
b) Sodium chloride (NaCl)
c) Ethanol (C2H5OH)
d) Glucose (C6H12O6)

Answer
b) Sodium chloride (NaCl)

The charge on one mole of electrons is approximately equal to:
a) +6.022 × 10^23 C
b) -6.022 × 10^23 C
c) +96,485 C
d) -96,485 C

Answer
c) +96,485 C

In an electrochemical cell, oxidation occurs at the:
a) Anode
b) Cathode
c) Electrolyte
d) External circuit

Answer
a) Anode

The standard reduction potential of any half-cell is measured with respect to the:
a) Anode
b) Cathode
c) Hydrogen electrode
d) Salt bridge

Answer
c) Hydrogen electrode

The reduction half-reaction involves the:
a) Gain of electrons
b) Loss of electrons
c) Formation of anions
d) Formation of cations

Answer
a) Gain of electrons

Which of the following is the correct representation of the cell notation for a galvanic cell involving copper and silver electrodes?
a) Cu | Ag || Cu(NO3)2 || AgNO3
b) Cu | Cu(NO3)2 || AgNO3 || Ag
c) Ag | AgNO3 || Cu(NO3)2 || Cu
d) Ag | Cu(NO3)2 || AgNO3 || Cu

Answer
c) Ag | AgNO3 || Cu(NO3)2 || Cu

The Nernst equation is used to calculate the cell potential under non-standard conditions by taking into account the concentrations of reactants and products and the:
a) Volume of the cell
b) Temperature of the cell
c) Pressure of the cell
d) Mass of the cell

Answer
b) Temperature of the cell

Which of the following substances is an oxidizing agent?
a) Hydrogen gas (H2)
b) Oxygen gas (O2)
c) Chlorine gas (Cl2)
d) Water (H2O)

Answer
c) Chlorine gas (Cl2)

The quantity of electricity required to deposit one mole of any substance is called:
a) Faraday’s law
b) Faraday’s constant
c) Electrochemical equivalent
d) Electrolysis constant

Answer
c) Electrochemical equivalent

Electrolysis is commonly used for the extraction of which metal from its ore?
a) Gold
b) Iron
c) Copper
d) Silver

Answer
c) Copper

Which of the following is a non-spontaneous reaction?
a) ∆G > 0
b) ∆G = 0
c) ∆G < 0
d) ∆G is not defined

Answer
a) ∆G > 0

The process of using a sacrificial metal to protect another metal from corrosion is known as:
a) Electrolysis
b) Cathodic protection
c) Anodic protection
d) Galvanic cell

Answer
b) Cathodic protection

Which of the following is used as the anode in a lead-acid battery?
a) Lead dioxide (PbO2)
b) Sulfuric acid (H2SO4)
c) Lead (P
b)
d) Carbon

Answer
c) Lead (Pb)

The standard hydrogen electrode (SHE) is assigned a standard reduction potential of:
a) +0.34 V
b) -0.34 V
c) +1.00 V
d) 0.00 V

Answer
d) 0.00 V

Which of the following is an example of an inert electrode?
a) Copper electrode
b) Platinum electrode
c) Zinc electrode
d) Iron electrode

Answer
b) Platinum electrode

The oxidation half-reaction involves the:
a) Gain of electrons
b) Loss of electrons
c) Formation of anions
d) Formation of cations

Answer
b) Loss of electrons

Which of the following is a strong electrolyte?
a) Acetic acid (CH3COOH)
b) Sodium chloride (NaCl)
c) Ethanol (C2H5OH)
d) Glucose (C6H12O6)

Answer
b) Sodium chloride (NaCl)

The charge on one mole of electrons is approximately equal to:
a) +6.022 × 10^23 C
b) -6.022 × 10^23 C
c) +96,485 C
d) -96,485 C

Answer
c) +96,485 C

In an electrochemical cell, oxidation occurs at the:
a) Anode
b) Cathode
c) Electrolyte
d) External circuit

Answer
a) Anode

The standard reduction potential of any half-cell is measured with respect to the:
a) Anode
b) Cathode
c) Hydrogen electrode
d) Salt bridge

Answer
c) Hydrogen electrode

The reduction half-reaction involves the:
a) Gain of electrons
b) Loss of electrons
c) Formation of anions
d) Formation of cations

Answer
a) Gain of electrons

Which of the following is the correct representation of the cell notation for a galvanic cell involving copper and silver electrodes?
a) Cu | Ag || Cu(NO3)2 || AgNO3
b) Cu | Cu(NO3)2 || AgNO3 || Ag
c) Ag | AgNO3 || Cu(NO3)2 || Cu
d) Ag | Cu(NO3)2 || AgNO3 || Cu

Answer
c) Ag | AgNO3 || Cu(NO3)2 || Cu

The Nernst equation is used to calculate the cell potential under non-standard conditions by taking into account the concentrations of reactants and products and the:
a) Volume of the cell
b) Temperature of the cell
c) Pressure of the cell
d) Mass of the cell

Answer
b) Temperature of the cell

Which of the following substances is an oxidizing agent?
a) Hydrogen gas (H2)
b) Oxygen gas (O2)
c) Chlorine gas (Cl2)
d) Water (H2O)

Answer
c) Chlorine gas (Cl2)

The quantity of electricity required to deposit one mole of any substance is called:
a) Faraday’s law
b) Faraday’s constant
c) Electrochemical equivalent
d) Electrolysis constant

Answer
c) Electrochemical equivalent

Electrolysis is commonly used for the extraction of which metal from its ore?
a) Gold
b) Iron
c) Copper
d) Silver

Answer
c) Copper

Which of the following is a non-spontaneous reaction?
a) ∆G > 0
b) ∆G = 0
c) ∆G < 0
d) ∆G is not defined

Answer
a) ∆G > 0

The process of using a sacrificial metal to protect another metal from corrosion is known as:
a) Electrolysis
b) Cathodic protection
c) Anodic protection
d) Galvanic cell

Answer
b) Cathodic protection

Which of the following is used as the anode in a lead-acid battery?
a) Lead dioxide (PbO2)
b) Sulfuric acid (H2SO4)
c) Lead (Pb)
d) Carbon

Answer
c) Lead (Pb)

The standard hydrogen electrode (SHE) is assigned a standard reduction potential of:
a) +0.34 V
b) -0.34 V
c) +1.00 V
d) 0.00 V

Answer
d) 0.00 V

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See Also  11th Class Chemistry Chapter 6 MCQs with Answers
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