NEET Chemistry: Some Basic Concepts Of Chemistry — MCQ Test 11

Q6. How many grams of \( \ce{Fe2O3} \) are required to produce 16.8 g of \( \ce{Fe} \) with excess \( \ce{CO} \)? (Molar masses: \( \ce{Fe2O3} \) = 160 g/mol, Fe = 56 g/mol)

Q7. A 1.5 L sample of a gas at STP contains 0.75 g of carbon and 0.25 g of hydrogen. What is its molecular formula? (Atomic masses: C = 12, H = 1)

Q8. A 0.42 g sample of a hydrocarbon produces 1.32 g of \( \ce{CO2} \) and 0.54 g of \( \ce{H2O} \) on complete combustion. What is its molecular formula if its molar mass is 42 g/mol? (Atomic masses: C = 12, H = 1, O = 16)

Q9. What is the mole fraction of \( \ce{CH3OH} \) in a solution containing 16 g of \( \ce{CH3OH} \) and 72 g of \( \ce{H2O} \)? (Molar masses: \( \ce{CH3OH} \) = 32 g/mol, \( \ce{H2O} \) = 18 g/mol)

Q10. A solution contains 10 ppm of \( \ce{K2SO4} \) by mass in water. What is its molality? (Molar mass: \( \ce{K2SO4} \) = 174 g/mol)

NEET Chemistry — Some Basic Concepts Of Chemistry

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A solution contains 20 ppm of \( \ce{K2SO4} \) by mass in water. What is its molarity if the density is 1 g/mL? (Molar mass: \( \ce{K2SO4} \) = 174 g/mol)

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About this NEET MCQ Test

This page provides a free online MCQ test for NEET Chemistry preparation, focusing specifically on the chapter Some Basic Concepts Of Chemistry. It contains 10 carefully selected multiple-choice questions (MCQs) designed to test your conceptual understanding and exam readiness.

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Key concepts covered in this specific test include Solution, Contains, Molarity, Hydrocarbon, Weighing, and Produces.

Taking these timed MCQ tests helps you simulate the real NEET exam environment. Detailed step-by-step explanations are provided for every question to help you learn from your mistakes and strengthen your fundamentals.

Preview of Questions in this Test

Q1. A solution contains 20 ppm of \( \ce{K2SO4} \) by mass in water. What is its molarity if the density is 1 g/mL? (Molar mass: \( \ce{K2SO4} \) = 174 g/mol)

  • A. 2.0 × 10⁻⁴ M
  • B. 1.0 × 10⁻⁴ M
  • C. 1.149 × 10⁻⁴ M
  • D. 5.0 × 10⁻⁵ M

Q2. A hydrocarbon (C and H only) weighing 0.26 g produces 0.88 g of \( \ce{CO2} \) and 0.18 g of \( \ce{H2O} \) on complete combustion. What is its molecular formula if its molar mass is 26 g/mol? (Atomic masses: C = 12, H = 1, O = 16)

  • A. \( \ce{C2H2} \)
  • B. \( \ce{CH4} \)
  • C. \( \ce{C2H4} \)
  • D. \( \ce{C3H6} \)

Q3. What volume of \( \ce{O2} \) at STP is required to burn 5 g of \( \ce{C2H5OH} \) completely to \( \ce{CO2} \) and \( \ce{H2O} \)? (Molar mass: \( \ce{C2H5OH} \) = 46 g/mol)

  • A. 7.3 L
  • B. 2.43 L
  • C. 14.6 L
  • D. 22.4 L

Q4. How many grams of \( \ce{HCl} \) are needed to react with 10 g of \( \ce{CaCO3} \) to produce 4.4 g of \( \ce{CO2} \)? (Molar masses: \( \ce{CaCO3} \) = 100 g/mol, \( \ce{HCl} \) = 36.5 g/mol, \( \ce{CO2} \) = 44 g/mol)

  • A. 3.65 g
  • B. 7.3 g
  • C. 14.6 g
  • D. 10 g

Q5. A 500 mL solution of \( \ce{KNO3} \) has a molarity of 0.4 M and a density of 1.01 g/mL. What is the mass percentage of \( \ce{KNO3} \)? (Molar mass: \( \ce{KNO3} \) = 101 g/mol)

  • A. 2%
  • B. 4%
  • C. 6%
  • D. 8%

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