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. If 10 g of sugar (C12H22O11) is dissolved in 200 g of water, what is the mass percent of the sugar solution? (2023)

A. 4.76%
B. 5.00%
C. 10.00%
D. 2.50%

Solution

Mass percent = (mass of solute / mass of solution) x 100. Mass of solution = 10 g + 200 g = 210 g. Mass percent = (10 g / 210 g) x 100 = 4.76%.

Correct Answer: A — 4.76%

Q. If 10 g of sugar (C12H22O11) is dissolved in 200 g of water, what is the mass percent of the solution? (Molar mass of sugar = 342 g/mol) (2023)

A. 4.76%
B. 5.00%
C. 10.00%
D. 2.50%

Solution

Mass percent = (mass of solute / mass of solution) x 100. Mass of solution = 10 g + 200 g = 210 g. Mass percent = (10 g / 210 g) x 100 = 4.76%.

Correct Answer: B — 5.00%

Q. If 10 g of sugar (C12H22O11) is dissolved in 200 g of water, what is the mass percent of the solution? (2023)

A. 4.76%
B. 5.00%
C. 10.00%
D. 20.00%

Solution

Mass percent = (mass of solute / mass of solution) × 100. Mass of solution = 10 g + 200 g = 210 g. Mass percent = (10 g / 210 g) × 100 = 4.76%.

Correct Answer: B — 5.00%

Q. If 10 g of sugar (C12H22O11) is dissolved in 200 g of water, what is the mass percent of the sugar solution? (Molar mass of sugar = 342 g/mol) (2023)

A. 4.76%
B. 5.00%
C. 10.00%
D. 2.50%

Solution

Mass percent = (mass of solute / mass of solution) × 100. Mass of solution = 10 g + 200 g = 210 g. Mass percent = (10 g / 210 g) × 100 = 4.76%.

Correct Answer: A — 4.76%

Q. If 10 g of sugar is dissolved in 100 g of water, what is the mass percent of sugar in the solution? (2023)

A. 10%
B. 5%
C. 20%
D. 15%

Solution

Mass percent = (mass of solute / total mass of solution) x 100. Total mass = 10 g + 100 g = 110 g. Mass percent = (10 g / 110 g) x 100 = 9.09%, approximately 10%.

Correct Answer: A — 10%

Q. If 10 g of sugar is dissolved in 100 g of water, what is the mass percentage of sugar in the solution? (2023)

A. 10%
B. 5%
C. 20%
D. 15%

Solution

Mass percentage = (mass of solute / mass of solution) × 100. Mass of solution = 10 g + 100 g = 110 g. Mass percentage = (10 g / 110 g) × 100 = 9.09%, approximately 10%.

Correct Answer: A — 10%

Q. If 10 grams of calcium carbonate (CaCO3) decomposes, how many grams of calcium oxide (CaO) are produced?

A. 5 g
B. 10 g
C. 8 g
D. 7 g

Solution

The balanced equation is CaCO3 → CaO + CO2. The molar mass of CaCO3 is 100 g/mol and CaO is 56 g/mol. Thus, 10 g of CaCO3 produces (10 g / 100 g/mol) x 56 g/mol = 5.6 g of CaO.

Correct Answer: C — 8 g

Q. If 10 grams of NaCl are dissolved in water, how many moles of NaCl are present? (Molar mass of NaCl = 58.5 g/mol)

A. 0.17 moles
B. 0.5 moles
C. 1.0 moles
D. 1.5 moles

Solution

Moles of NaCl = mass (g) / molar mass (g/mol) = 10 g / 58.5 g/mol = 0.171 moles.

Correct Answer: A — 0.17 moles

Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the concentration in g/L? (2020)

A. 20 g/L
B. 10 g/L
C. 5 g/L
D. 15 g/L

Solution

Concentration = (10 g / 0.5 L) = 20 g/L.

Correct Answer: A — 20 g/L

Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the concentration in grams per liter? (2022)

A. 10 g/L
B. 20 g/L
C. 5 g/L
D. 15 g/L

Solution

Concentration = mass/volume = 10 g / 0.5 L = 20 g/L.

Correct Answer: A — 10 g/L

Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the mass/volume percent concentration?

A. 1%
B. 2%
C. 5%
D. 10%

Solution

Mass/volume percent = (mass of solute / volume of solution) x 100 = (10 g / 500 mL) x 100 = 2%.

Correct Answer: B — 2%

Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the mass/volume percent concentration? (2020) 2020

A. 2%
B. 5%
C. 10%
D. 20%

Solution

Mass/volume % = (mass of solute / volume of solution) * 100 = (10 g / 500 mL) * 100 = 2%.

Correct Answer: B — 5%

Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the molality of the solution? (Molar mass of NaCl = 58.5 g/mol)

A. 0.34 m
B. 0.17 m
C. 0.85 m
D. 0.50 m

Solution

Molality (m) = moles of solute / kg of solvent. Moles of NaCl = 10 g / 58.5 g/mol = 0.171 moles. Mass of water = 0.5 kg. Molality = 0.171 moles / 0.5 kg = 0.342 m.

Correct Answer: A — 0.34 m

Q. If 10 grams of NaCl is dissolved in enough water to make 500 mL of solution, what is the molality of the solution? (Molar mass of NaCl = 58.5 g/mol)

A. 0.34 m
B. 0.17 m
C. 0.85 m
D. 0.50 m

Solution

Moles of NaCl = 10 g / 58.5 g/mol = 0.171 moles. Mass of solvent (water) = 0.5 kg. Molality (m) = moles of solute / kg of solvent = 0.171 moles / 0.5 kg = 0.34 m.

Correct Answer: A — 0.34 m

Q. If 10 grams of NaOH are dissolved in water, how many moles of NaOH are present? (Molar mass of NaOH = 40 g/mol)

A. 0.25 moles
B. 0.5 moles
C. 1 mole
D. 2.5 moles

Solution

To find the number of moles, use the formula: moles = mass/molar mass. Thus, 10 g / 40 g/mol = 0.25 moles.

Correct Answer: B — 0.5 moles

Q. If 10 grams of NaOH is dissolved in 500 mL of solution, what is the molality of the solution? (Molar mass of NaOH = 40 g/mol)

A. 0.5 m
B. 1 m
C. 2 m
D. 0.25 m

Solution

Moles of NaOH = 10 g / 40 g/mol = 0.25 moles. Mass of solvent (water) = 0.5 kg. Molality (m) = moles of solute / kg of solvent = 0.25 moles / 0.5 kg = 0.5 m.

Correct Answer: B — 1 m

Q. If 10 grams of NaOH is dissolved in enough water to make 500 mL of solution, what is the molarity of the solution? (Molar mass of NaOH = 40 g/mol)

A. 0.5 M
B. 1 M
C. 2 M
D. 0.25 M

Solution

Moles of NaOH = 10 g / 40 g/mol = 0.25 moles. Molarity = 0.25 moles / 0.5 L = 0.5 M.

Correct Answer: B — 1 M

Q. If 10 grams of sodium chloride (NaCl) is dissolved in 100 mL of water, what is the concentration in g/L?

A. 100 g/L
B. 10 g/L
C. 1 g/L
D. 0.1 g/L

Solution

Concentration = (10 g / 0.1 L) = 100 g/L.

Correct Answer: A — 100 g/L

Q. If 10 liters of a solution contains 30% salt, how much salt is present in the solution?

A. 3 liters
B. 2 liters
C. 4 liters
D. 1 liter

Solution

30% of 10 liters = 0.3 * 10 = 3 liters of salt.

Correct Answer: A — 3 liters

Q. If 10 liters of paint can cover 200 square meters, how many liters are needed to cover 500 square meters?

A. 20 liters
B. 25 liters
C. 30 liters
D. 35 liters

Solution

10 liters cover 200 m², so 1 liter covers 20 m². For 500 m², needed = 500 / 20 = 25 liters.

Correct Answer: B — 25 liters

Q. If 10 men can complete a work in 15 days, how many days will it take for 5 men to complete the same work?

A. 20 days
B. 25 days
C. 30 days
D. 35 days

Solution

If 10 men take 15 days, then 5 men will take (10 * 15) / 5 = 30 days.

Correct Answer: C — 30 days

Q. If 10 mL of a 0.1 M NaOH solution is mixed with 10 mL of a 0.1 M HCl solution, what will be the resulting pH?

A. 0
B. 7
C. 14
D. 3

Solution

The NaOH and HCl neutralize each other, resulting in a neutral solution with a pH of 7.

Correct Answer: B — 7

Q. If 10 students can complete a project in 15 days, how many days will it take for 5 students to complete the same project?

A. 20 days
B. 25 days
C. 30 days
D. 35 days

Solution

Work = 10 students * 15 days = 150 student-days. For 5 students, days = 150 student-days / 5 students = 30 days.

Correct Answer: C — 30 days

Q. If 10 workers can finish a job in 15 days, how many days will it take for 5 workers to finish the same job?

A. 30 days
B. 35 days
C. 40 days
D. 45 days

Solution

If 10 workers take 15 days, then 5 workers will take 15 * 10 / 5 = 30 days.

Correct Answer: C — 40 days

Q. If 100 g of glucose (C6H12O6) is dissolved in 1 L of solution, what is the molarity of the solution? (Molar mass of glucose = 180 g/mol)

A. 0.56 M
B. 1.0 M
C. 0.33 M
D. 0.75 M

Solution

Moles of glucose = 100 g / 180 g/mol = 0.556 moles. Molarity = moles of solute / liters of solution = 0.556 moles / 1 L = 0.56 M.

Correct Answer: A — 0.56 M

Q. If 100 g of water at 0°C is mixed with 100 g of water at 100°C, what will be the final temperature of the mixture?

A. 50°C
B. 25°C
C. 75°C
D. 0°C

Solution

Using the principle of conservation of energy, the final temperature will be 50°C.

Correct Answer: A — 50°C

Q. If 100 g of water at 0°C is mixed with 100 g of water at 100°C, what will be the final temperature?

A. 50°C
B. 25°C
C. 75°C
D. 0°C

Solution

The final temperature will be 50°C due to equal masses and specific heat capacities.

Correct Answer: A — 50°C

Q. If 100 g of water at 80°C is mixed with 200 g of water at 20°C, what will be the final temperature?

A. 30°C
B. 40°C
C. 50°C
D. 60°C

Solution

Using the principle of conservation of energy, the final temperature can be calculated to be 40°C.

Correct Answer: B — 40°C

Q. If 100 J of heat is added to a system and 40 J of work is done by the system, what is the change in internal energy?

A. 60 J
B. 40 J
C. 100 J
D. 140 J

Solution

According to the First Law of Thermodynamics, ΔU = Q - W. Here, ΔU = 100 J - 40 J = 60 J.

Correct Answer: A — 60 J

Q. If 100 J of heat is added to a system at a constant temperature of 300 K, what is the change in entropy?

A. 0.33 J/K
B. 0.25 J/K
C. 0.5 J/K
D. 0.75 J/K

Solution

The change in entropy ΔS = Q/T = 100 J / 300 K = 0.33 J/K.

Correct Answer: A — 0.33 J/K

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