Major Competitive Exams

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Major Competitive Exams

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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!

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Q. What is the square root of the complex number -4? (2020)

A. 2i
B. -2i
C. 4i
D. -4i

Solution

The square root of -4 is √(-1) * √4 = 2i.

Correct Answer: A — 2i

Q. What is the standard acceleration due to gravity in m/s²?

A. 9.8
B. 10
C. 9.81
D. 9.75

Solution

The standard acceleration due to gravity is approximately 9.81 m/s².

Correct Answer: C — 9.81

Q. What is the standard deviation of the data set {10, 12, 23, 23, 16, 23, 21, 16}?

A. 5
B. 6
C. 4
D. 3

Solution

Mean = 19.5, Variance = 25, Standard Deviation = √25 = 5.

Correct Answer: A — 5

Q. What is the standard deviation of the data set {10, 12, 23, 23, 16, 23, 21}?

A. 5.5
B. 4.5
C. 6.5
D. 3.5

Solution

Mean = 19.14, Variance = 20.25, Standard Deviation = √20.25 = 4.5.

Correct Answer: B — 4.5

Q. What is the standard deviation of the data set {4, 8, 6, 5, 3}?

A. 1.58
B. 2.58
C. 3.58
D. 4.58

Solution

Mean = 5.2. Variance = [(4-5.2)² + (8-5.2)² + (6-5.2)² + (5-5.2)² + (3-5.2)²]/5 = 6.56. Standard Deviation = √6.56 ≈ 2.56.

Correct Answer: B — 2.58

Q. What is the standard deviation of the data set: 1, 2, 3, 4, 5?

A. 1
B. 1.5
C. 2
D. 2.5

Solution

Mean = 3. Standard Deviation = sqrt[((1-3)^2 + (2-3)^2 + (3-3)^2 + (4-3)^2 + (5-3)^2)/5] = sqrt[2] = 1.414.

Correct Answer: A — 1

Q. What is the standard electrode potential of the half-reaction Zn²⁺ + 2e⁻ → Zn?

A. 0.76 V
B. 0.34 V
C. -0.76 V
D. -0.34 V

Solution

The standard electrode potential for Zn²⁺/Zn is -0.76 V.

Correct Answer: C — -0.76 V

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

Solution

The standard electrode potential of the hydrogen electrode is defined as 0.00 V.

Correct Answer: A — 0.00 V

Q. What is the standard electrode potential of the hydrogen electrode? (2023) 2023

A. 0 V
B. 1 V
C. 2 V
D. 0.5 V

Solution

The standard electrode potential of the hydrogen electrode is defined as 0 V.

Correct Answer: A — 0 V

Q. What is the standard enthalpy change (ΔH°) for the formation of water from its elements? (2022)

A. -285.83 kJ/mol
B. 0 kJ/mol
C. 285.83 kJ/mol
D. -241.82 kJ/mol

Solution

The standard enthalpy change for the formation of water from its elements (H2 and O2) is -285.83 kJ/mol.

Correct Answer: A — -285.83 kJ/mol

Q. What is the standard enthalpy change (ΔH°) for the reaction: C(s) + O2(g) → CO2(g)? (2022)

A. It is always positive.
B. It is always negative.
C. It can be zero.
D. It depends on the temperature.

Solution

The standard enthalpy change for combustion reactions, such as the formation of CO2 from carbon and oxygen, is typically negative, indicating that the reaction is exothermic.

Correct Answer: B — It is always negative.

Q. What is the standard enthalpy change for the formation of a compound?

A. ΔHf
B. ΔHc
C. ΔHrxn
D. ΔHsol

Solution

The standard enthalpy change for the formation of a compound is denoted as ΔHf.

Correct Answer: A — ΔHf

Q. What is the standard enthalpy change for the formation of an element in its standard state?

A. Zero
B. Positive
C. Negative
D. Depends on the element

Solution

The standard enthalpy change for the formation of an element in its standard state is defined as zero.

Correct Answer: A — Zero

Q. What is the standard enthalpy change for the formation of water from its elements?

A. -285.83 kJ/mol
B. -241.82 kJ/mol
C. -393.5 kJ/mol
D. -572.4 kJ/mol

Solution

The standard enthalpy change for the formation of water (H2 + 1/2 O2 -> H2O) is -285.83 kJ/mol.

Correct Answer: A — -285.83 kJ/mol

Q. What is the standard enthalpy change for the reaction 2H2 + O2 → 2H2O if the enthalpy of formation of H2O is -285.8 kJ/mol?

A. -571.6 kJ
B. -285.8 kJ
C. 0 kJ
D. 285.8 kJ

Solution

ΔH = 2 * (-285.8 kJ) = -571.6 kJ

Correct Answer: A — -571.6 kJ

Q. What is the standard enthalpy change for the reaction 2H2(g) + O2(g) → 2H2O(l)?

A. -285.83 kJ/mol
B. -241.82 kJ/mol
C. -572.4 kJ/mol
D. -1000 kJ/mol

Solution

The standard enthalpy of formation of water is -241.82 kJ/mol.

Correct Answer: B — -241.82 kJ/mol

Q. What is the standard enthalpy change for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) if ΔHf°(NH3) = -45.9 kJ/mol?

A. -91.8 kJ
B. 0 kJ
C. 45.9 kJ
D. 91.8 kJ

Solution

ΔH = 2 * ΔHf°(NH3) = 2 * (-45.9) = -91.8 kJ

Correct Answer: A — -91.8 kJ

Q. What is the standard enthalpy change for the reaction: C(s) + O2(g) → CO2(g) if ΔHf° for CO2 is -393.5 kJ/mol?

A. -393.5 kJ
B. 0 kJ
C. 393.5 kJ
D. None of the above

Solution

The standard enthalpy change is equal to the enthalpy of formation of CO2, which is -393.5 kJ.

Correct Answer: A — -393.5 kJ

Q. What is the standard enthalpy change of formation for a substance?

A. The enthalpy change when one mole of a compound is formed from its elements in their standard states.
B. The enthalpy change when one mole of a substance is completely burned in oxygen.
C. The enthalpy change when one mole of a substance is dissolved in water.
D. The enthalpy change when one mole of a gas is compressed to a smaller volume.

Solution

The standard enthalpy change of formation is defined as the enthalpy change when one mole of a compound is formed from its elements in their standard states.

Correct Answer: A — The enthalpy change when one mole of a compound is formed from its elements in their standard states.

Q. What is the standard enthalpy change of formation for an element in its standard state?

A. 0 kJ/mol
B. 100 kJ/mol
C. 298 kJ/mol
D. 1 kJ/mol

Solution

The standard enthalpy change of formation for an element in its standard state is defined as 0 kJ/mol.

Correct Answer: A — 0 kJ/mol

Q. What is the standard enthalpy change of formation for elements in their standard state?

A. 0 kJ/mol
B. 100 kJ/mol
C. 298 kJ/mol
D. 1 kJ/mol

Solution

The standard enthalpy change of formation for elements in their standard state is defined as zero.

Correct Answer: A — 0 kJ/mol

Q. What is the standard enthalpy change of formation for water (H2O) at 25°C?

A. -285.83 kJ/mol
B. -241.82 kJ/mol
C. -393.5 kJ/mol
D. -241.0 kJ/mol

Solution

The standard enthalpy change of formation for water at 25°C is -241.82 kJ/mol.

Correct Answer: B — -241.82 kJ/mol

Q. What is the standard enthalpy of formation for an element in its standard state?

A. 0 kJ/mol
B. 100 kJ/mol
C. 298 kJ/mol
D. 1 kJ/mol

Solution

The standard enthalpy of formation for an element in its standard state is defined as 0 kJ/mol.

Correct Answer: A — 0 kJ/mol

Q. What is the standard enthalpy of formation for elements in their standard state?

A. 0 kJ/mol
B. 1 kJ/mol
C. 100 kJ/mol
D. Not defined

Solution

The standard enthalpy of formation for elements in their standard state is defined as 0 kJ/mol.

Correct Answer: A — 0 kJ/mol

Q. What is the standard entropy change (ΔS°) for the reaction: 2 SO2(g) + O2(g) → 2 SO3(g)?

A. Positive
B. Negative
C. Zero
D. Cannot be determined

Solution

The reaction decreases the number of gas molecules from 3 to 2, leading to a decrease in disorder and thus a negative ΔS°.

Correct Answer: B — Negative

Q. What is the standard entropy change (ΔS°) for the reaction: 2H2(g) + O2(g) → 2H2O(g)?

A. Positive
B. Negative
C. Zero
D. Cannot be determined

Solution

The reaction results in a decrease in the number of gas molecules (from 3 to 2), leading to a negative change in entropy.

Correct Answer: B — Negative

Q. What is the standard entropy change (ΔS°) for the reaction: 2SO2(g) + O2(g) → 2SO3(g)?

A. Increases
B. Decreases
C. Remains constant
D. Cannot be determined

Solution

The reaction decreases the number of gas molecules from 3 to 2, leading to a decrease in entropy.

Correct Answer: B — Decreases

Q. What is the standard form of the equation of a parabola that opens upwards with vertex at the origin?

A. y^2 = 4ax
B. x^2 = 4ay
C. y^2 = -4ax
D. x^2 = -4ay

Solution

The standard form of a parabola that opens upwards is given by x^2 = 4ay.

Correct Answer: B — x^2 = 4ay

Q. What is the standard Gibbs Free Energy change (ΔG°) for a reaction at standard conditions?

A. Always zero
B. Depends on the reaction
C. Is a constant value
D. Is always positive

Solution

ΔG° depends on the specific reaction and its conditions.

Correct Answer: B — Depends on the reaction

Q. What is the standard molar entropy of a substance?

A. Entropy at 0 K
B. Entropy at 25 °C and 1 atm
C. Entropy at boiling point
D. Entropy at melting point

Solution

Standard molar entropy is defined as the entropy of 1 mole of a substance at 25 °C and 1 atm pressure.

Correct Answer: B — Entropy at 25 °C and 1 atm

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