NEET Chemistry: Thermodynamics — MCQ Test 6

Q6. For the process \(H_2O(l) \rightarrow H_2O(g)\) at 373 K, \(\Delta H = 40.79 \, \text{kJ/mol}\), what is \(\Delta S_{surr}\)?

Q7. The standard enthalpy of formation of \(NH_3(g)\) is -46.1 kJ/mol. What is \(\Delta H\) for \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\)?

Q8. For an ideal gas expanding reversibly and adiabatically, the relationship between temperature and volume is:

Q9. For the reaction \( 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \), \( \Delta H = -483.6 \, \text{kJ/mol} \) at 298 K. What is \( \Delta U \)? (\( R = 8.314 \, \text{J/mol·K} \))

Q10. A reaction has \(\Delta H = -100 \, \text{kJ}\) and \(\Delta S = -200 \, \text{J/K}\). At what temperature does it become spontaneous?

NEET Chemistry — Thermodynamics

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The work done in the reversible adiabatic expansion of 1 mol of an ideal gas from 10 L to 20 L is (\( \gamma = 1.4 \)) at 300 K. Calculate \( w \). (\( R = 8.314 \, \text{J/mol·K} \))

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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 Reversible, Adiabatic, Expansion, Calculate, Following, and Spontaneous.

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. The work done in the reversible adiabatic expansion of 1 mol of an ideal gas from 10 L to 20 L is (\( \gamma = 1.4 \)) at 300 K. Calculate \( w \). (\( R = 8.314 \, \text{J/mol·K} \))

  • A. 1509.2 J
  • B. 0 J
  • C. -1509.2 J
  • D. -2494.0 J

Q2. Which of the following is always true for a spontaneous process at constant temperature and pressure?

  • A. \(\Delta G < 0\)
  • B. \(\Delta H < 0\)
  • C. \(\Delta S > 0\)
  • D. \(\Delta U < 0\)

Q3. Calculate \(\Delta S_{surr}\) when 2 mol of a substance melts at 300 K if \(\Delta H_{fus} = 8 \, \text{kJ/mol}\).

  • A. 53.33 J/K
  • B. 8 J/K
  • C. -53.33 J/K
  • D. -26.67 J/K

Q4. A reaction has \( \Delta H = 80.00 \, \text{kJ/mol} \), \( \Delta S = 200.0 \, \text{J/K·mol} \), and is spontaneous at 450 K. What is \( \Delta G \) at 450 K?

  • A. 10 kJ/mol
  • B. 90 kJ/mol
  • C. -10 kJ/mol
  • D. -80 kJ/mol

Q5. Calculate \(\Delta H\) for the reaction \(C(s) + 2H_2(g) \rightarrow CH_4(g)\) given: \(CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)\), \(\Delta H = -890.3 \, \text{kJ/mol}\); \(C(s) + O_2(g) \rightarrow CO_2(g)\), \(\Delta H = -393.5 \, \text{kJ/mol}\); \(H_2(g) + \frac{1}{2}O_2(g) \rightarrow H_2O(l)\), \(\Delta H = -285.8 \, \text{kJ/mol}\).

  • A. 74.8 kJ/mol
  • B. -74.8 kJ/mol
  • C. -890.3 kJ/mol
  • D. -52.3 kJ/mol

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