NEET Chemistry: Some Basic Concepts Of Chemistry — MCQ Test 7

Q6. A 0.5 L sample of a gas at STP weighs 0.67 g and contains only carbon and hydrogen. If it produces 1.32 g of \( \ce{CO2} \) on burning, what is its molecular formula? (Atomic masses: C = 12, H = 1)

Q7. A 0.70 g sample of a hydrocarbon produces 2.20 g of \( \ce{CO2} \) and 0.90 g of \( \ce{H2O} \) on complete combustion. What is its molecular formula if its molar mass is 70 g/mol? (Atomic masses: C = 12, H = 1, O = 16)

Q8. A 0.2 M \( \ce{NaCl} \) solution is diluted by adding 150 mL of water to 50 mL of the original solution. What is the final molarity?

Q9. A compound contains 24% magnesium, 28% sulfur, and 48% oxygen by mass. What is its empirical formula? (Atomic masses: Mg = 24, S = 32, O = 16)

Q10. A mixture of 4 g \( \ce{H2} \) and 56 g \( \ce{N2} \) is used to synthesize \( \ce{NH3} \). What is the maximum mass of \( \ce{NH3} \) produced? (Molar masses: \( \ce{H2} \) = 2 g/mol, \( \ce{N2} \) = 28 g/mol, \( \ce{NH3} \) = 17 g/mol)

NEET Chemistry — Some Basic Concepts Of Chemistry

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What volume of \( \ce{N2} \) at STP is required to react with 4 g of \( \ce{H2} \) to produce \( \ce{NH3} \) with 100% yield? (Molar mass: \( \ce{H2} \) = 2 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 Required, Occupies, Produced, Contains, Hydrogen, 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. What volume of \( \ce{N2} \) at STP is required to react with 4 g of \( \ce{H2} \) to produce \( \ce{NH3} \) with 100% yield? (Molar mass: \( \ce{H2} \) = 2 g/mol)

  • A. 14.93 L
  • B. 22.4 L
  • C. 7.47 L
  • D. 29.86 L

Q2. A gas occupies 4.48 L at STP and weighs 6.4 g. What is its molar mass?

  • A. 16 g/mol
  • B. 48 g/mol
  • C. 32 g/mol
  • D. 28 g/mol

Q3. What is the mass of water produced when 8 g of \( \ce{CH4} \) reacts with 24 g of \( \ce{O2} \)? (Atomic masses: C = 12, H = 1, O = 16)

  • A. 9 g
  • B. 13.5 g
  • C. 18 g
  • D. 12 g

Q4. A 2 L sample of a gas at STP weighs 1.4 g and contains only carbon and hydrogen. If it produces 4.4 g of \( \ce{CO2} \) on burning, what is its molecular formula? (Atomic masses: C = 12, H = 1)

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

Q5. What is the mass percentage of \( \ce{NH4Cl} \) in a solution made by dissolving 10.7 g of \( \ce{NH4Cl} \) in 39.3 g of water? (Molar mass: \( \ce{NH4Cl} \) = 53.5 g/mol)

  • A. 20%
  • B. 25%
  • C. 21.4%
  • D. 15%

+ 5 more questions in the actual test

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