NEET Chemistry: Some Basic Concepts Of Chemistry — MCQ Test 16

Q6. What volume of \( \ce{N2} \) at STP is required to react with 6 g of \( \ce{H2} \) to produce \( \ce{NH3} \) with 60% yield? (Molar mass: \( \ce{H2} \) = 2 g/mol)

Q7. What mass of \( \ce{N2} \) reacts with 6 g of \( \ce{H2} \) to form \( \ce{NH3} \), if \( \ce{H2} \) is the limiting reagent? (Molar masses: \( \ce{N2} \) = 28 g/mol, \( \ce{H2} \) = 2 g/mol)

Q8. A 400 mL solution contains 14.6 g of \( \ce{HCl} \) and has a density of 1.02 g/mL. What is its molarity? (Molar mass: \( \ce{HCl} \) = 36.5 g/mol)

Q9. What volume of \( \ce{CO2} \) at STP is produced when 10 g of \( \ce{C4H10} \) is burned completely? (Molar mass: \( \ce{C4H10} \) = 58 g/mol)

Q10. A mixture of 10 g \( \ce{C} \) and 24 g \( \ce{O2} \) is ignited to form \( \ce{CO2} \). What is the mass of \( \ce{CO2} \) produced? (Atomic masses: C = 12, O = 16)

NEET Chemistry — Some Basic Concepts Of Chemistry

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A solution contains 10 ppm of \( \ce{SO2} \) by mass in water. What is the molarity if the density of the solution is 1 g/mL? (Molar mass: \( \ce{SO2} \) = 64 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, Produces, and Complete.

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 10 ppm of \( \ce{SO2} \) by mass in water. What is the molarity if the density of the solution is 1 g/mL? (Molar mass: \( \ce{SO2} \) = 64 g/mol)

  • A. 1.0 × 10⁻⁴ M
  • B. 2.0 × 10⁻⁴ M
  • C. 1.5625 × 10⁻⁴ M
  • D. 5.0 × 10⁻⁴ M

Q2. A 0.84 g sample of a hydrocarbon produces 2.64 g of \( \ce{CO2} \) and 1.08 g of \( \ce{H2O} \) on complete combustion. What is its molecular formula if its molar mass is 84 g/mol? (Atomic masses: C = 12, H = 1, O = 16)

  • A. \( \ce{C6H12} \)
  • B. \( \ce{C5H10} \)
  • C. \( \ce{C4H8} \)
  • D. \( \ce{C3H6} \)

Q3. A gas occupies 3.36 L at STP and weighs 4.8 g. What is its molar mass?

  • A. 16 g/mol
  • B. 48 g/mol
  • C. 32 g/mol
  • D. 24 g/mol

Q4. How many grams of \( \ce{Na2SO4} \) are produced when 8 g of \( \ce{NaOH} \) reacts with excess \( \ce{H2SO4} \)? (Molar masses: \( \ce{NaOH} \) = 40 g/mol, \( \ce{Na2SO4} \) = 142 g/mol)

  • A. 7.1 g
  • B. 14.2 g
  • C. 28.4 g
  • D. 10.6 g

Q5. 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)

  • A. \( \ce{C3H6} \)
  • B. \( \ce{C2H4} \)
  • C. \( \ce{C4H8} \)
  • D. \( \ce{C5H10} \)

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