NEET Chemistry: Thermodynamics — MCQ Test 18

Q6. In a reversible isothermal compression of 2 mol of an ideal gas at 300 K, the work done is 4988 J. What is the heat absorbed? (\(R = 8.314 \, \text{J/mol·K}\))

Q7. Calculate \(\Delta S_{surr}\) when 3 mol of a liquid freezes at 250 K if \(\Delta H_{fus} = 5.5 \, \text{kJ/mol}\).

Q8. Calculate the bond enthalpy of \(C-C\) in \(C_2H_6(g)\) given: \(\Delta H_f^\circ (C_2H_6,g) = -84.7 \, \text{kJ/mol}\), \(\Delta H_a (C,g) = 715 \, \text{kJ/mol}\), \(\Delta H_a (H,g) = 218 \, \text{kJ/mol}\), \(C-H = 413 \, \text{kJ/mol}\).

Q9. The enthalpy of formation of \(NO_2(g)\) is 33.2 kJ/mol. What is \(\Delta H\) for \(N_2(g) + 2O_2(g) \rightarrow 2NO_2(g)\)?

Q10. Calculate \(\Delta H\) for \(C(s) + H_2(g) + O_2(g) \rightarrow CH_3OH(l)\) given: \(CH_3OH(l) + \frac{3}{2}O_2(g) \rightarrow CO_2(g) + 2H_2O(l)\), \(\Delta H = -726.5 \, \text{kJ/mol}\); \(C(s) + O_2(g) \rightarrow CO_2(g)\), \(\Delta H = -393.5 \, \text{kJ/mol}\); \(H_2(g) + \frac{1}{2}O_2(g) \rightarrow H_2O(l)\), \(\Delta H = -285.8 \, \text{kJ/mol}\).

NEET Chemistry — Thermodynamics

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1Question 1 of 10
Medium

Calculate \( \Delta S_{surr} \) for the combustion of 1 mol of \( CH_4(g) \) at 298 K, given \( \Delta H = -890.00 \, \text{kJ/mol} \).

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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 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 Calculate, Combustion, Releases, Reaction, Temperature, and Enthalpy.

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. Calculate \( \Delta S_{surr} \) for the combustion of 1 mol of \( CH_4(g) \) at 298 K, given \( \Delta H = -890.00 \, \text{kJ/mol} \).

  • A. -2986.6 J/K
  • B. 890 J/K
  • C. -890 J/K
  • D. 2986.6 J/K

Q2. A system releases 200 J of heat and has 150 J of work done on it. What is \(\Delta U\)?

  • A. 350 J
  • B. -50 J
  • C. 50 J
  • D. -350 J

Q3. For a reaction with \(\Delta H = -50 \, \text{kJ}\) and \(\Delta S = 100 \, \text{J/K}\), at what temperature is \(\Delta G = 0\)?

  • A. 250 K
  • B. 1000 K
  • C. 500 K
  • D. 50 K

Q4. The enthalpy change for the process \(H_2O(s) \rightarrow H_2O(l)\) is:

  • A. \(\Delta H_{vap}\)
  • B. \(\Delta H_{fus}\)
  • C. \(-\Delta H_{fus}\)
  • D. \(\Delta H_{comb}\)

Q5. For an exothermic reaction with \( \Delta H = -100.00 \, \text{kJ/mol} \) and \( \Delta n_g = -1 \) at 298 K, what is \( \Delta U \)? (\( R = 8.314 \, \text{J/mol·K} \))

  • A. -100 kJ
  • B. -97.5 kJ
  • C. -102.5 kJ
  • D. -95 kJ

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