NEET Chemistry: Thermodynamics — MCQ Test 5

Q6. A system at constant pressure absorbs 1000 J of heat and expands by 0.4 L against 2.5 atm. What is \(\Delta U\)? (1 atm·L = 101.3 J)

Q7. Calculate \(\Delta H\) for \(CH_4(g) \rightarrow C(g) + 4H(g)\) using: \(\Delta H_f^\circ (CH_4,g) = -74.8 \, \text{kJ/mol}\), \(\Delta H_a (C,g) = 715 \, \text{kJ/mol}\), \(\Delta H_a (H,g) = 218 \, \text{kJ/mol}\).

Q8. Calculate \(\Delta G^\circ\) for a reaction with \(K = 2.5 \times 10^{-3}\) at 298 K. (\(R = 8.314 \, \text{J/mol·K}\))

Q9. What is the work done when 2 mol of an ideal gas expands isothermally and reversibly from 5 L to 10 L at 300 K? (\(R = 8.314 \, \text{J/mol·K}\))

Q10. For an ideal gas (\(\gamma = 1.33\)) expanding adiabatically from 8 L to 16 L at 500 K, what is the final temperature?

NEET Chemistry — Thermodynamics

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In a process, 300 J of heat is absorbed by a system, and 100 J of work is done on the system. What is \(\Delta U\)?

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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 Thermodynamics. 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 Absorbed, Performs, Internal, Vaporization, Surroundings, and Constant.

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. In a process, 300 J of heat is absorbed by a system, and 100 J of work is done on the system. What is \(\Delta U\)?

  • A. 400 J
  • B. 200 J
  • C. -400 J
  • D. 100 J

Q2. A system absorbs 500 J of heat and performs 200 J of work. What is the change in internal energy (\(\Delta U\))?

  • A. 300 J
  • B. 700 J
  • C. -300 J
  • D. 200 J

Q3. What is the change in internal energy (\( \Delta U \)) for the vaporization of 1 mol of water at 373 K if \( \Delta H = 40.79 \, \text{kJ/mol} \)? (\( R = 8.314 \, \text{J/mol·K} \))

  • A. 40.79 kJ/mol
  • B. 37.69 kJ/mol
  • C. 43.89 kJ/mol
  • D. 34.60 kJ/mol

Q4. A system absorbs 1200 J of heat and does 500 J of work on the surroundings at constant pressure. What is \(\Delta H\)?

  • A. 1200 J
  • B. 700 J
  • C. 1700 J
  • D. -700 J

Q5. Calculate \( \Delta S_{sys} \) when 1 mol of water vaporizes at 373 K. (\( \Delta H_{vap} = 40.79 \, \text{kJ/mol} \))

  • A. 40.79 J/K
  • B. 80.00 J/K
  • C. 109.4 J/K
  • D. 150.0 J/K

+ 5 more questions in the actual test

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