Q. In a Daniell cell, which electrode is the anode?
-
A.
Copper electrode
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B.
Zinc electrode
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C.
Silver electrode
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D.
Lead electrode
Solution
In a Daniell cell, the zinc electrode acts as the anode where oxidation occurs, releasing electrons.
Correct Answer:
B
— Zinc electrode
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Q. In a galvanic cell, what occurs at the anode?
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A.
Reduction of the oxidizing agent.
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B.
Oxidation of the reducing agent.
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C.
Neutralization of acids.
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D.
Formation of a precipitate.
Solution
In a galvanic cell, oxidation occurs at the anode, where the reducing agent loses electrons.
Correct Answer:
B
— Oxidation of the reducing agent.
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Q. In electrolysis, what happens to the ions in the electrolyte?
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A.
They remain unchanged.
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B.
They are oxidized or reduced at the electrodes.
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C.
They evaporate into gas.
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D.
They form a solid precipitate.
Solution
During electrolysis, ions in the electrolyte are oxidized or reduced at the electrodes, leading to chemical changes.
Correct Answer:
B
— They are oxidized or reduced at the electrodes.
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Q. In electroplating, what is the purpose of the metal ions in the solution?
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A.
To provide a source of electrons
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B.
To deposit metal onto a surface
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C.
To increase conductivity
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D.
To act as a catalyst
Solution
In electroplating, metal ions in the solution are reduced at the cathode, depositing metal onto the surface.
Correct Answer:
B
— To deposit metal onto a surface
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Q. What is the primary use of a fuel cell?
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A.
To store energy
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B.
To convert chemical energy into electrical energy
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C.
To measure temperature
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D.
To catalyze reactions
Solution
A fuel cell converts the chemical energy of a fuel (like hydrogen) directly into electrical energy through electrochemical reactions.
Correct Answer:
B
— To convert chemical energy into electrical energy
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Q. What is the role of a cathode in an electrochemical cell?
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A.
It is where oxidation occurs.
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B.
It is where reduction occurs.
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C.
It is where the salt bridge connects.
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D.
It is where the electrons are generated.
Solution
The cathode is the electrode where reduction occurs, gaining electrons from the external circuit.
Correct Answer:
B
— It is where reduction occurs.
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Q. What is the role of a salt bridge in an electrochemical cell?
-
A.
To connect the two electrodes
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B.
To maintain charge balance
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C.
To increase conductivity
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D.
To provide a source of ions
Solution
The salt bridge maintains charge balance by allowing ions to flow between the two half-cells, preventing charge buildup.
Correct Answer:
B
— To maintain charge balance
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Q. What is the significance of the Faraday constant in electrochemistry?
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A.
It relates to the energy of a reaction.
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B.
It defines the charge of one mole of electrons.
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C.
It measures the temperature of a reaction.
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D.
It indicates the speed of a reaction.
Solution
The Faraday constant represents the charge of one mole of electrons, approximately 96485 C/mol.
Correct Answer:
B
— It defines the charge of one mole of electrons.
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Q. What is the standard electrode potential of a half-reaction?
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A.
The potential at which the reaction occurs at standard conditions
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B.
The potential at which the reaction occurs at any conditions
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C.
The potential difference between two electrodes
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D.
The energy change of the reaction
Solution
The standard electrode potential is the voltage measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C).
Correct Answer:
A
— The potential at which the reaction occurs at standard conditions
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Q. Which of the following describes a primary battery?
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A.
It can be recharged multiple times.
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B.
It is designed for single-use only.
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C.
It has a longer lifespan than secondary batteries.
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D.
It operates at higher voltages.
Solution
A primary battery is designed for single-use and cannot be recharged, unlike secondary batteries.
Correct Answer:
B
— It is designed for single-use only.
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Q. Which of the following is a common application of electrolysis?
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A.
Water splitting
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B.
Photosynthesis
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C.
Combustion
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D.
Fermentation
Solution
Electrolysis is commonly used for water splitting to produce hydrogen and oxygen gases.
Correct Answer:
A
— Water splitting
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Q. Which of the following is a real-world application of electrochemistry?
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A.
Photosynthesis in plants.
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B.
Corrosion prevention techniques.
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C.
Thermal energy storage.
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D.
Mechanical work in engines.
Solution
Corrosion prevention techniques, such as cathodic protection, are practical applications of electrochemistry.
Correct Answer:
B
— Corrosion prevention techniques.
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Q. Which of the following statements about corrosion is true?
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A.
It is a spontaneous redox reaction
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B.
It requires an external power source
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C.
It only occurs in acidic environments
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D.
It is always a slow process
Solution
Corrosion is a spontaneous redox reaction where metals oxidize, often leading to deterioration.
Correct Answer:
A
— It is a spontaneous redox reaction
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