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XII_CHEMISTRY_NEW_CHAPTER-02: ELECTROCHEMISTRY _ A&R TEST ITEMS [SYLLABUS TOPIC-WISE]
# Correct Assertion Correct Reason
ALL CONCEPTS IN THE CHAPTER
Conductance increases with an increase in the As concentration increases, more ions are available for conduction,
1
concentration of the electrolyte. elevating conductance.
Kohlrausch’s Law sums the individual contributions It assumes ions contribute proportionally to conductivity,
2
of anion and cation to molar conductivity. elucidating the law's essence.
Electrolysis of water forms hydrogen at the cathode Electric current decomposes water into its elemental gases,
3
and oxygen at the anode. elucidating the electrolysis process.
First law of electrolysis: substance production is It follows mass conservation and electron transfer, fundamental to
4
proportional to electricity passed. understanding electrolysis.
Dry cells are non-rechargeable due to irreversible Irreversible reactions prevent cell recharge, distinguishing dry cells
5
internal chemical reactions. from rechargeable ones.
Galvanic cells convert chemical energy into electrical Through redox reactions, galvanic cells generate a potential
6
energy. difference for work, elucidating their energy conversion.
EMF of a cell is the maximum work when no current It signifies potential difference under standard conditions without
7
flows through it. current flow, elucidating EMF.
Standard electrode potential of hydrogen is 0 V, By convention, hydrogen’s potential serves as the zero reference
8
serving as a reference point. for other potentials, essential in electrochemistry.
Gibbs energy change is negative for spontaneous cell It indicates spontaneity, crucial for understanding reaction
9
reactions. feasibility, elucidating Gibbs energy's role.
Fuel cells directly convert stored fuel energy into They utilize electrochemical reactions for direct energy conversion,
10
electricity. fundamental to fuel cell function.
Metals corrode via electrochemical oxidation in the Electrochemical processes in water with oxygen cause metal
11
presence of water and oxygen. oxidation, elucidating corrosion mechanisms.
Lead accumulators utilize a reversible lead-lead oxide The reversible reaction enables storage and release of electrical
12
redox reaction for recharging. energy, distinguishing lead accumulators.
Concept 1. Redox reactions: [Definition and examples of redox reactions, Oxidation number, Balancing redox reactions, and
Types of redox reactions (combination, decomposition, displacement)]
In a redox reaction, oxidation and reduction occur Electron transfer results in simultaneous oxidation and reduction,
13
simultaneously. depicting redox reactions.
An increase in the oxidation number of an atom Oxidation involves electron loss, whereas reduction entails electron
14 indicates oxidation, while a decrease indicates gain, revealing oxidation number changes.
reduction.
Balancing a redox reaction requires equating Electron conservation is crucial in redox reactions, necessitating
15 electrons lost in oxidation with those gained in balance between oxidation and reduction steps.
reduction.
Redox reactions can be classified into three types: The nature of reactants and products determines redox reaction
16
combination, decomposition, and displacement. types, leading to distinct classifications.
In a combination reaction, two or more substances Combination reactions involve electron gain, hence are classified as
17
combine to form a single product. redox reactions, explaining product formation.
Decomposition reactions involve the breakdown of a Electron loss characterizes decomposition reactions, hence their
18
single reactant into two or more products. classification as redox reactions, elucidating product formation.
Displacement reactions involve the replacement of Displacement occurs when a more reactive element replaces a less
19
one element in a compound with another element. reactive one, defining the reaction type.
Redox reactions play an essential role in the Metal corrosion involves oxidation of the metal and reduction of
20 corrosion of metals. other substances, emphasizing the significance of redox reactions.
Redox reactions are critical in biological systems, Cellular respiration oxidizes glucose for energy and photosynthesis
21 such as cellular respiration and photosynthesis. reduces carbon dioxide for glucose production, showcasing their
biological significance.
The oxidation number of oxygen in a compound is Oxygen, being electronegative, typically gains electrons in
22
usually -2. reactions, determining its oxidation state.
The sum of oxidation numbers in a neutral compound Neutral compounds have a net charge of zero, reflecting balance in
23
is zero. oxidation numbers, ensuring charge neutrality.
Redox reactions can be used to generate electricity in Electron transfer in electrochemical cells produces current,
24 electrochemical cells. facilitating work, showcasing their utility in electricity generation.
Concept 2. Conductance in electrolytic solutions: [Definition of electrolytes and non-electrolytes, Conductivity and resistivity,
Specific and molar conductivity, Variation of conductivity with concentration, and, Kohlrausch's Law]
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XII_CHEMISTRY_NEW_CHAPTER-02: ELECTROCHEMISTRY _ A&R TEST ITEMS [SYLLABUS TOPIC-WISE]
# Correct Assertion Correct Reason
ALL CONCEPTS IN THE CHAPTER
Conductance increases with an increase in the As concentration increases, more ions are available for conduction,
1
concentration of the electrolyte. elevating conductance.
Kohlrausch’s Law sums the individual contributions It assumes ions contribute proportionally to conductivity,
2
of anion and cation to molar conductivity. elucidating the law's essence.
Electrolysis of water forms hydrogen at the cathode Electric current decomposes water into its elemental gases,
3
and oxygen at the anode. elucidating the electrolysis process.
First law of electrolysis: substance production is It follows mass conservation and electron transfer, fundamental to
4
proportional to electricity passed. understanding electrolysis.
Dry cells are non-rechargeable due to irreversible Irreversible reactions prevent cell recharge, distinguishing dry cells
5
internal chemical reactions. from rechargeable ones.
Galvanic cells convert chemical energy into electrical Through redox reactions, galvanic cells generate a potential
6
energy. difference for work, elucidating their energy conversion.
EMF of a cell is the maximum work when no current It signifies potential difference under standard conditions without
7
flows through it. current flow, elucidating EMF.
Standard electrode potential of hydrogen is 0 V, By convention, hydrogen’s potential serves as the zero reference
8
serving as a reference point. for other potentials, essential in electrochemistry.
Gibbs energy change is negative for spontaneous cell It indicates spontaneity, crucial for understanding reaction
9
reactions. feasibility, elucidating Gibbs energy's role.
Fuel cells directly convert stored fuel energy into They utilize electrochemical reactions for direct energy conversion,
10
electricity. fundamental to fuel cell function.
Metals corrode via electrochemical oxidation in the Electrochemical processes in water with oxygen cause metal
11
presence of water and oxygen. oxidation, elucidating corrosion mechanisms.
Lead accumulators utilize a reversible lead-lead oxide The reversible reaction enables storage and release of electrical
12
redox reaction for recharging. energy, distinguishing lead accumulators.
Concept 1. Redox reactions: [Definition and examples of redox reactions, Oxidation number, Balancing redox reactions, and
Types of redox reactions (combination, decomposition, displacement)]
In a redox reaction, oxidation and reduction occur Electron transfer results in simultaneous oxidation and reduction,
13
simultaneously. depicting redox reactions.
An increase in the oxidation number of an atom Oxidation involves electron loss, whereas reduction entails electron
14 indicates oxidation, while a decrease indicates gain, revealing oxidation number changes.
reduction.
Balancing a redox reaction requires equating Electron conservation is crucial in redox reactions, necessitating
15 electrons lost in oxidation with those gained in balance between oxidation and reduction steps.
reduction.
Redox reactions can be classified into three types: The nature of reactants and products determines redox reaction
16
combination, decomposition, and displacement. types, leading to distinct classifications.
In a combination reaction, two or more substances Combination reactions involve electron gain, hence are classified as
17
combine to form a single product. redox reactions, explaining product formation.
Decomposition reactions involve the breakdown of a Electron loss characterizes decomposition reactions, hence their
18
single reactant into two or more products. classification as redox reactions, elucidating product formation.
Displacement reactions involve the replacement of Displacement occurs when a more reactive element replaces a less
19
one element in a compound with another element. reactive one, defining the reaction type.
Redox reactions play an essential role in the Metal corrosion involves oxidation of the metal and reduction of
20 corrosion of metals. other substances, emphasizing the significance of redox reactions.
Redox reactions are critical in biological systems, Cellular respiration oxidizes glucose for energy and photosynthesis
21 such as cellular respiration and photosynthesis. reduces carbon dioxide for glucose production, showcasing their
biological significance.
The oxidation number of oxygen in a compound is Oxygen, being electronegative, typically gains electrons in
22
usually -2. reactions, determining its oxidation state.
The sum of oxidation numbers in a neutral compound Neutral compounds have a net charge of zero, reflecting balance in
23
is zero. oxidation numbers, ensuring charge neutrality.
Redox reactions can be used to generate electricity in Electron transfer in electrochemical cells produces current,
24 electrochemical cells. facilitating work, showcasing their utility in electricity generation.
Concept 2. Conductance in electrolytic solutions: [Definition of electrolytes and non-electrolytes, Conductivity and resistivity,
Specific and molar conductivity, Variation of conductivity with concentration, and, Kohlrausch's Law]
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