Major Competitive Exams MCQ & Objective Questions
Major Competitive Exams play a crucial role in shaping the academic and professional futures of students in India. These exams not only assess knowledge but also test problem-solving skills and time management. Practicing MCQs and objective questions is essential for scoring better, as they help in familiarizing students with the exam format and identifying important questions that frequently appear in tests.
What You Will Practise Here
Key concepts and theories related to major subjects
Important formulas and their applications
Definitions of critical terms and terminologies
Diagrams and illustrations to enhance understanding
Practice questions that mirror actual exam patterns
Strategies for solving objective questions efficiently
Time management techniques for competitive exams
Exam Relevance
The topics covered under Major Competitive Exams are integral to various examinations such as CBSE, State Boards, NEET, and JEE. Students can expect to encounter a mix of conceptual and application-based questions that require a solid understanding of the subjects. Common question patterns include multiple-choice questions that test both knowledge and analytical skills, making it essential to be well-prepared with practice MCQs.
Common Mistakes Students Make
Rushing through questions without reading them carefully
Overlooking the negative marking scheme in MCQs
Confusing similar concepts or terms
Neglecting to review previous years’ question papers
Failing to manage time effectively during the exam
FAQs
Question: How can I improve my performance in Major Competitive Exams?Answer: Regular practice of MCQs and understanding key concepts will significantly enhance your performance.
Question: What types of questions should I focus on for these exams?Answer: Concentrate on important Major Competitive Exams questions that frequently appear in past papers and mock tests.
Question: Are there specific strategies for tackling objective questions?Answer: Yes, practicing under timed conditions and reviewing mistakes can help develop effective strategies.
Start your journey towards success by solving practice MCQs today! Test your understanding and build confidence for your upcoming exams. Remember, consistent practice is the key to mastering Major Competitive Exams!
Q. What is the energy stored in a capacitor of capacitance 4μF charged to 12V? (2022)
A.
24μJ
B.
28.8μJ
C.
48μJ
D.
72μJ
Show solution
Solution
The energy stored (U) is given by U = 1/2 CV². Thus, U = 1/2 * 4μF * (12V)² = 288μJ.
Correct Answer:
C
— 48μJ
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Q. What is the energy stored in a capacitor of capacitance 5μF charged to a potential difference of 10V? (2023)
A.
0.25mJ
B.
0.5mJ
C.
0.75mJ
D.
1mJ
Show solution
Solution
Using the formula U = 1/2 CV², we have U = 1/2 * 5μF * (10V)² = 0.5mJ.
Correct Answer:
B
— 0.5mJ
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Q. What is the energy stored in a capacitor of capacitance C charged to a potential V? (2021)
A.
CV
B.
1/2 CV^2
C.
1/2 QV
D.
QV
Show solution
Solution
The energy (U) stored in a capacitor is given by the formula U = 1/2 CV^2.
Correct Answer:
B
— 1/2 CV^2
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Q. What is the energy stored in a capacitor of capacitance C charged to a voltage V?
A.
1/2 CV
B.
CV
C.
1/2 C/V
D.
C/V
Show solution
Solution
The energy (U) stored in a capacitor is given by the formula U = 1/2 CV².
Correct Answer:
A
— 1/2 CV
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Q. What is the energy stored in a capacitor with capacitance C charged to a voltage V?
A.
1/2 CV²
B.
CV
C.
1/2 V²/C
D.
C²V
Show solution
Solution
The energy (U) stored in a capacitor is given by the formula U = 1/2 CV².
Correct Answer:
A
— 1/2 CV²
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Q. What is the energy stored in a capacitor with capacitance C charged to voltage V?
A.
1/2 CV
B.
CV
C.
1/2 C/V
D.
C/V
Show solution
Solution
The energy (U) stored in a capacitor is given by the formula U = 1/2 CV².
Correct Answer:
A
— 1/2 CV
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Q. What is the enthalpy change for the formation of 1 mole of CO2 from its elements in their standard states?
A.
-393.5 kJ/mol
B.
-285.8 kJ/mol
C.
0 kJ/mol
D.
100 kJ/mol
Show solution
Solution
The standard enthalpy of formation of CO2 is -393.5 kJ/mol.
Correct Answer:
A
— -393.5 kJ/mol
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Q. What is the enthalpy change for the formation of water from hydrogen and oxygen?
A.
It is positive.
B.
It is negative.
C.
It is zero.
D.
It is undefined.
Show solution
Solution
The formation of water from hydrogen and oxygen is an exothermic reaction, resulting in a negative enthalpy change.
Correct Answer:
B
— It is negative.
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Q. What is the enthalpy change for the reaction 2Na + Cl2 → 2NaCl?
A.
-411 kJ
B.
-240 kJ
C.
0 kJ
D.
411 kJ
Show solution
Solution
The enthalpy change for the formation of NaCl from its elements is -411 kJ.
Correct Answer:
A
— -411 kJ
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Q. What is the enthalpy change for the reaction at constant pressure?
A.
ΔH = ΔU + PΔV
B.
ΔH = ΔU - PΔV
C.
ΔH = ΔU + VΔP
D.
ΔH = ΔU - VΔP
Show solution
Solution
At constant pressure, the enthalpy change is given by ΔH = ΔU + PΔV.
Correct Answer:
A
— ΔH = ΔU + PΔV
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Q. What is the enthalpy change for the reaction N2(g) + 3H2(g) → 2NH3(g) at standard conditions?
A.
-92.4 kJ
B.
-45.9 kJ
C.
0 kJ
D.
0.5 kJ
Show solution
Solution
The standard enthalpy change for the formation of ammonia is -92.4 kJ.
Correct Answer:
A
— -92.4 kJ
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Q. What is the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(g)?
A.
It is positive.
B.
It is negative.
C.
It is zero.
D.
It is dependent on temperature.
Show solution
Solution
The formation of water from hydrogen and oxygen is an exothermic reaction, thus the enthalpy change is negative.
Correct Answer:
B
— It is negative.
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Q. What is the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)?
A.
-571.6 kJ
B.
-285.8 kJ
C.
0 kJ
D.
285.8 kJ
Show solution
Solution
The enthalpy change for the formation of 2 moles of water is -571.6 kJ.
Correct Answer:
A
— -571.6 kJ
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Q. What is the enthalpy change for the reaction: C(s) + O2(g) -> CO2(g)?
A.
-393.5 kJ/mol
B.
-241.8 kJ/mol
C.
0 kJ/mol
D.
285.8 kJ/mol
Show solution
Solution
The enthalpy change for the formation of CO2 from carbon and oxygen is -393.5 kJ/mol.
Correct Answer:
A
— -393.5 kJ/mol
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Q. What is the enthalpy change for the reaction: C(s) + O2(g) → CO2(g)?
A.
-393.5 kJ/mol
B.
-241.8 kJ/mol
C.
0 kJ/mol
D.
285.8 kJ/mol
Show solution
Solution
The enthalpy change for the formation of CO2 from its elements is -393.5 kJ/mol.
Correct Answer:
A
— -393.5 kJ/mol
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Q. What is the enthalpy change for the reaction: CaCO3(s) → CaO(s) + CO2(g)?
A.
It is an endothermic reaction.
B.
It is an exothermic reaction.
C.
It has no enthalpy change.
D.
It is spontaneous at all temperatures.
Show solution
Solution
The decomposition of calcium carbonate is an endothermic reaction, requiring heat input.
Correct Answer:
A
— It is an endothermic reaction.
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Q. What is the enthalpy change for the reaction: H2(g) + 1/2 O2(g) → H2O(l)?
A.
-285.8 kJ/mol
B.
0 kJ/mol
C.
-241.8 kJ/mol
D.
-572 kJ/mol
Show solution
Solution
The standard enthalpy change for the formation of water from its elements is -241.8 kJ/mol.
Correct Answer:
C
— -241.8 kJ/mol
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Q. What is the enthalpy change for the reaction: N2(g) + 3H2(g) → 2NH3(g)?
A.
It is always positive.
B.
It is always negative.
C.
It can be either positive or negative depending on conditions.
D.
It is zero.
Show solution
Solution
The formation of ammonia from nitrogen and hydrogen is an exothermic reaction, thus the enthalpy change is negative.
Correct Answer:
B
— It is always negative.
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Q. What is the enthalpy change when 1 mole of NaCl is dissolved in water?
A.
-3.87 kJ
B.
0 kJ
C.
+3.87 kJ
D.
-7.0 kJ
Show solution
Solution
The enthalpy change when 1 mole of NaCl is dissolved in water is approximately -3.87 kJ.
Correct Answer:
A
— -3.87 kJ
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Q. What is the enthalpy change when 1 mole of water vapor condenses to liquid water?
A.
It is positive.
B.
It is negative.
C.
It is zero.
D.
It is dependent on pressure.
Show solution
Solution
The condensation of water vapor to liquid water releases heat, making the enthalpy change negative.
Correct Answer:
B
— It is negative.
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Q. What is the entropy change for a reversible isothermal expansion of an ideal gas?
A.
nR ln(Vf/Vi)
B.
0
C.
nR(Tf - Ti)
D.
nC ln(Vf/Vi)
Show solution
Solution
The entropy change for a reversible isothermal expansion of an ideal gas is ΔS = nR ln(Vf/Vi).
Correct Answer:
A
— nR ln(Vf/Vi)
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Q. What is the entropy change for a reversible isothermal process?
A.
Zero
B.
nR ln(Vf/Vi)
C.
nR(Tf - Ti)
D.
nR ln(Tf/Ti)
Show solution
Solution
The entropy change for a reversible isothermal process is ΔS = nR ln(Vf/Vi).
Correct Answer:
B
— nR ln(Vf/Vi)
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Q. What is the entropy change for a reversible process?
A.
Always positive
B.
Always negative
C.
Can be zero
D.
Depends on the path taken
Show solution
Solution
For a reversible process, the entropy change can be zero if the process is isothermal and reversible.
Correct Answer:
C
— Can be zero
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Q. What is the entropy change for a system that undergoes a phase transition at constant temperature?
A.
ΔS = 0
B.
ΔS = Q/T
C.
ΔS = T/Q
D.
ΔS = Q + T
Show solution
Solution
During a phase transition at constant temperature, the change in entropy is given by ΔS = Q/T, where Q is the heat absorbed or released.
Correct Answer:
B
— ΔS = Q/T
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Q. What is the entropy change for an ideal gas during an isothermal expansion?
A.
Zero
B.
nR ln(Vf/Vi)
C.
nC_v ln(Tf/Ti)
D.
nC_p ln(Tf/Ti)
Show solution
Solution
The entropy change for an ideal gas during an isothermal expansion is ΔS = nR ln(Vf/Vi).
Correct Answer:
B
— nR ln(Vf/Vi)
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Q. What is the entropy change for the isothermal expansion of an ideal gas from volume V1 to V2 at temperature T?
A.
R ln(V2/V1)
B.
R (V2 - V1)/T
C.
0
D.
R (V1/V2)
Show solution
Solution
The entropy change for an isothermal expansion is given by ΔS = nR ln(V2/V1). For 1 mole, ΔS = R ln(V2/V1).
Correct Answer:
A
— R ln(V2/V1)
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Q. What is the entropy change for the mixing of two ideal gases at constant temperature?
A.
0
B.
R ln(2)
C.
R ln(V1/V2)
D.
R ln(V1*V2)
Show solution
Solution
The entropy change for the mixing of two ideal gases at constant temperature is ΔS = nR ln(2) for equal moles of each gas.
Correct Answer:
B
— R ln(2)
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Q. What is the entropy change when 1 mole of an ideal gas is heated at constant volume from temperature T1 to T2?
A.
R ln(T2/T1)
B.
R (T2 - T1)
C.
0
D.
R (T1/T2)
Show solution
Solution
The change in entropy at constant volume is given by ΔS = nC_v ln(T2/T1). For 1 mole, ΔS = R ln(T2/T1).
Correct Answer:
A
— R ln(T2/T1)
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Q. What is the entropy change when 1 mole of an ideal gas is heated at constant volume?
A.
0
B.
R ln(T2/T1)
C.
R (T2 - T1)
D.
R (T1/T2)
Show solution
Solution
The change in entropy when heating an ideal gas at constant volume is given by ΔS = nC_v ln(T2/T1). For 1 mole, it simplifies to ΔS = R ln(T2/T1).
Correct Answer:
B
— R ln(T2/T1)
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Q. What is the entropy change when 1 mole of ice at 0°C is converted to water at 0°C?
A.
0 J/K
B.
R ln(2)
C.
R
D.
Positive value
Show solution
Solution
The phase change from ice to water at 0°C involves an increase in disorder, thus resulting in a positive change in entropy.
Correct Answer:
D
— Positive value
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