NEET Chemistry: Some Basic Concepts Of Chemistry — MCQ Test 18

Q6. How many significant figures are present in the result of \( \frac{0.0456 \times 273.15}{0.0821} \)?

Q7. A 0.5 M solution of \( \ce{NaOH} \) is diluted from 200 mL to 1 L. What is the new molarity?

Q8. What is the mass of \( \ce{CaSO4} \) produced when 13.6 g of \( \ce{Ca(OH)2} \) reacts with excess \( \ce{H2SO4} \)? (Molar masses: \( \ce{Ca(OH)2} \) = 74 g/mol, \( \ce{CaSO4} \) = 136 g/mol)

Q9. How many grams of \( \ce{CuO} \) are required to produce 6.4 g of \( \ce{Cu} \) with excess \( \ce{CO} \)? (Molar masses: \( \ce{CuO} \) = 79.5 g/mol, Cu = 64 g/mol)

Q10. How many grams of \( \ce{K2CO3} \) are required to produce 13.8 g of \( \ce{KCl} \) with excess \( \ce{HCl} \)? (Molar masses: \( \ce{K2CO3} \) = 138 g/mol, \( \ce{KCl} \) = 74.5 g/mol)

NEET Chemistry — Some Basic Concepts Of Chemistry

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What is the mole fraction of \( \ce{C2H5OH} \) in a solution containing 23 g of \( \ce{C2H5OH} \) and 18 g of \( \ce{H2O} \)? (Molar masses: \( \ce{C2H5OH} \) = 46 g/mol, \( \ce{H2O} \) = 18 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 Fraction, Solution, Containing, 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. What is the mole fraction of \( \ce{C2H5OH} \) in a solution containing 23 g of \( \ce{C2H5OH} \) and 18 g of \( \ce{H2O} \)? (Molar masses: \( \ce{C2H5OH} \) = 46 g/mol, \( \ce{H2O} \) = 18 g/mol)

  • A. 0.25
  • B. 0.333
  • C. 0.5
  • D. 0.67

Q2. A 0.54 g sample of a hydrocarbon produces 1.76 g of \( \ce{CO2} \) and 0.36 g of \( \ce{H2O} \) on complete combustion. If its molar mass is 54 g/mol, what is its molecular formula? (Atomic masses: C = 12, H = 1, O = 16)

  • A. \( \ce{C4H4} \)
  • B. \( \ce{C3H6} \)
  • C. \( \ce{C2H2} \)
  • D. \( \ce{C5H10} \)

Q3. What is the mole fraction of \( \ce{H2O} \) in a solution containing 9 g of \( \ce{H2O} \) and 23 g of \( \ce{C2H5OH} \)? (Molar masses: \( \ce{H2O} \) = 18 g/mol, \( \ce{C2H5OH} \) = 46 g/mol)

  • A. 0.25
  • B. 0.5
  • C. 0.75
  • D. 0.33

Q4. What is the mole fraction of \( \ce{CH3OH} \) in a solution containing 16 g of \( \ce{CH3OH} \) and 36 g of \( \ce{H2O} \)? (Molar masses: \( \ce{CH3OH} \) = 32 g/mol, \( \ce{H2O} \) = 18 g/mol)

  • A. 0.25
  • B. 0.2
  • C. 0.33
  • D. 0.5

Q5. A 1.5 L sample of a gas at STP weighs 2.1 g and contains only carbon and hydrogen. If it produces 2.64 g of \( \ce{CO2} \) on burning, what is its molecular formula? (Atomic masses: C = 12, H = 1)

  • A. \( \ce{CH4} \)
  • B. \( \ce{C2H4} \)
  • C. \( \ce{C3H8} \)
  • D. \( \ce{C2H6} \)

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