Q. In a concentration cell, the potential difference arises due to:
A.
Different temperatures
B.
Different concentrations
C.
Different pressures
D.
Different materials
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Solution
In a concentration cell, the potential difference arises due to different concentrations of the same species.
Correct Answer:
B
— Different concentrations
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Q. In a Daniell cell, which metal is oxidized?
A.
Copper
B.
Zinc
C.
Lead
D.
Silver
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Solution
In a Daniell cell, zinc is oxidized.
Correct Answer:
B
— Zinc
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Q. In a galvanic cell, the anode is where:
A.
Reduction occurs
B.
Oxidation occurs
C.
Electrons are gained
D.
The salt bridge is located
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Solution
In a galvanic cell, oxidation occurs at the anode.
Correct Answer:
B
— Oxidation occurs
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Q. In electrochemistry, what does the term 'reduction' refer to?
A.
Loss of electrons
B.
Gain of electrons
C.
Loss of protons
D.
Gain of protons
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Solution
Reduction refers to the gain of electrons in a chemical reaction.
Correct Answer:
B
— Gain of electrons
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Q. What is the effect of increasing temperature on the cell potential according to the Nernst equation?
A.
Increases cell potential
B.
Decreases cell potential
C.
No effect
D.
Depends on the reaction
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Solution
The effect of increasing temperature on cell potential depends on the reaction and its enthalpy change.
Correct Answer:
D
— Depends on the reaction
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Q. What is the effect of increasing temperature on the cell potential?
A.
Increases
B.
Decreases
C.
Remains constant
D.
Depends on the reaction
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Solution
The effect of temperature on cell potential depends on the reaction and its enthalpy change.
Correct Answer:
D
— Depends on the reaction
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Q. What is the main function of a salt bridge in a galvanic cell?
A.
To provide a path for electrons
B.
To maintain charge balance
C.
To increase voltage
D.
To decrease resistance
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Solution
The main function of a salt bridge is to maintain charge balance by allowing ions to flow.
Correct Answer:
B
— To maintain charge balance
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Q. What is the Nernst equation used for?
A.
Calculating pH
B.
Determining cell potential
C.
Finding molarity
D.
Measuring temperature
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Solution
The Nernst equation is used to determine the cell potential under non-standard conditions.
Correct Answer:
B
— Determining cell potential
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Q. What is the primary function of a cathode in an electrochemical cell?
A.
To oxidize species
B.
To reduce species
C.
To provide electrons
D.
To balance charge
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Solution
The cathode is where reduction occurs, gaining electrons in the process.
Correct Answer:
B
— To reduce species
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Q. What is the primary function of a salt bridge in a galvanic cell?
A.
To provide a path for electrons
B.
To maintain charge balance
C.
To increase voltage
D.
To decrease resistance
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Solution
The primary function of a salt bridge is to maintain charge balance by allowing ions to flow between the half-cells.
Correct Answer:
B
— To maintain charge balance
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Q. What is the primary reaction occurring in a lead-acid battery during discharge?
A.
Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O
B.
PbSO4 + 2H2O → Pb + PbO2 + 2H2SO4
C.
2Pb + 2H2SO4 → 2PbSO4 + H2
D.
PbO2 + 2H2SO4 → Pb + 2H2O + O2
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Solution
During discharge, the primary reaction in a lead-acid battery is Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O.
Correct Answer:
A
— Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O
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Q. What is the role of a salt bridge in a galvanic cell?
A.
To provide a pathway for electrons
B.
To maintain charge balance
C.
To increase voltage
D.
To decrease resistance
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Solution
The salt bridge maintains charge balance by allowing ions to flow between the two half-cells.
Correct Answer:
B
— To maintain charge balance
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Q. What is the role of the cathode in an electrochemical cell?
A.
Oxidation occurs
B.
Reduction occurs
C.
Electrons are lost
D.
Ions are produced
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Solution
In an electrochemical cell, reduction occurs at the cathode.
Correct Answer:
B
— Reduction occurs
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Q. What is the standard electrode potential of the hydrogen electrode?
A.
0.00 V
B.
0.34 V
C.
1.23 V
D.
0.76 V
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Solution
The standard electrode potential of the hydrogen electrode is defined as 0.00 V.
Correct Answer:
A
— 0.00 V
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Q. What is the unit of electric charge?
A.
Volt
B.
Ampere
C.
Coulomb
D.
Ohm
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Solution
The unit of electric charge is the Coulomb.
Correct Answer:
C
— Coulomb
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Q. What is the unit of electrical charge?
A.
Volt
B.
Ampere
C.
Coulomb
D.
Ohm
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Solution
The unit of electrical charge is the Coulomb.
Correct Answer:
C
— Coulomb
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Q. Which of the following is a characteristic of a fuel cell?
A.
Produces heat
B.
Converts chemical energy directly to electrical energy
C.
Requires combustion
D.
Is a type of battery
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Solution
A fuel cell converts chemical energy directly to electrical energy without combustion.
Correct Answer:
B
— Converts chemical energy directly to electrical energy
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Q. Which of the following is a primary cell?
A.
Lead-acid battery
B.
Nickel-cadmium battery
C.
Zinc-carbon battery
D.
Lithium-ion battery
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Solution
The zinc-carbon battery is a primary cell, while the others are secondary cells.
Correct Answer:
C
— Zinc-carbon battery
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Q. Which of the following metals can be used as an anode in a Daniell cell?
A.
Copper
B.
Zinc
C.
Silver
D.
Lead
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Solution
Zinc is used as the anode in a Daniell cell.
Correct Answer:
B
— Zinc
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Q. Which of the following metals can be used as an anode in electrolysis?
A.
Copper
B.
Gold
C.
Aluminum
D.
Silver
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Solution
Aluminum is commonly used as an anode in electrolysis due to its high reactivity.
Correct Answer:
C
— Aluminum
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Q. Which of the following metals cannot be used as an anode in a galvanic cell?
A.
Zinc
B.
Copper
C.
Lead
D.
Silver
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Solution
Copper cannot be used as an anode in a galvanic cell because it is less reactive than zinc.
Correct Answer:
B
— Copper
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Q. Which of the following statements is true about electrolysis?
A.
It requires a spontaneous reaction
B.
It is an endothermic process
C.
It involves the decomposition of a compound
D.
It occurs in a galvanic cell
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Solution
Electrolysis involves the decomposition of a compound using electrical energy.
Correct Answer:
C
— It involves the decomposition of a compound
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Q. Which of the following statements is true about electrolytic cells?
A.
They produce electrical energy
B.
They require an external power source
C.
They operate spontaneously
D.
They are always exothermic
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Solution
Electrolytic cells require an external power source to drive the non-spontaneous reactions.
Correct Answer:
B
— They require an external power source
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Showing 1 to 23 of 23 (1 Pages)
Electrochemistry MCQ & Objective Questions
Electrochemistry is a vital topic in the study of chemistry, especially for students preparing for school and competitive exams. Understanding electrochemical principles not only enhances conceptual clarity but also significantly boosts your exam performance. Practicing MCQs and objective questions in this area is essential, as it helps in identifying important concepts and improves problem-solving skills, ultimately leading to better scores.
What You Will Practise Here
Fundamentals of electrochemical cells and their types
Key concepts of oxidation and reduction reactions
Electrochemical series and its applications
Nernst equation and its significance in calculations
Standard electrode potentials and their importance
Applications of electrochemistry in real-life scenarios
Diagrams of galvanic and electrolytic cells
Exam Relevance
Electrochemistry is frequently featured in various examinations, including CBSE, State Boards, NEET, and JEE. Students can expect questions that test their understanding of electrochemical concepts, calculations involving the Nernst equation, and the ability to interpret electrochemical cells. Common question patterns include direct application of formulas, conceptual MCQs, and problem-solving scenarios that require a deep understanding of the subject.
Common Mistakes Students Make
Confusing oxidation and reduction processes in reactions
Misapplying the Nernst equation in calculations
Overlooking the significance of standard electrode potentials
Failing to interpret diagrams of electrochemical cells correctly
FAQs
Question: What is the Nernst equation used for?Answer: The Nernst equation is used to calculate the cell potential of an electrochemical cell under non-standard conditions.
Question: How do I identify oxidation and reduction in a reaction?Answer: Oxidation involves the loss of electrons, while reduction involves the gain of electrons. Identifying changes in oxidation states can help clarify these processes.
Ready to enhance your understanding of electrochemistry? Dive into our practice MCQs and test your knowledge on important Electrochemistry questions for exams. The more you practice, the more confident you will become!
