NEET Chemistry: Thermodynamics — MCQ Test 1

Q6. The enthalpy of combustion of glucose is -2808 kJ/mol. How much heat is released when 90 g of glucose is burnt? (Molar mass of \(C_6H_{12}O_6 = 180 \, \text{g/mol}\))

Q7. Calculate \(\Delta H\) for \(C(s) + \frac{1}{2}O_2(g) \rightarrow CO(g)\) given: \(C(s) + O_2(g) \rightarrow CO_2(g)\), \(\Delta H = -393.5 \, \text{kJ/mol}\); \(CO(g) + \frac{1}{2}O_2(g) \rightarrow CO_2(g)\), \(\Delta H = -283 \, \text{kJ/mol}\).

Q8. The equilibrium constant for a reaction is 100 at 300 K. Calculate \(\Delta G^\circ\). (\(R = 8.314 \, \text{J/mol·K}\))

Q9. Calculate the work done when 1 mol of an ideal gas expands isothermally and reversibly from 5 atm to 1 atm at 300 K. (\(R = 8.314 \, \text{J/mol·K}\))

Q10. Calculate the heat required to raise the temperature of 40 g of water from 25°C to 35°C. (Specific heat of water = 4.18 J/g·K)

NEET Chemistry — Thermodynamics

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Calculate \(\Delta S_{surr}\) when 2 mol of water freezes at 273 K if \(\Delta H_{fus} = 6.01 \, \text{kJ/mol}\).

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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, Undergoing, Reversible, Adiabatic, Compression, and Relationship.

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 \(\Delta S_{surr}\) when 2 mol of water freezes at 273 K if \(\Delta H_{fus} = 6.01 \, \text{kJ/mol}\).

  • A. -44.03 J/K
  • B. 22.01 J/K
  • C. 6.01 J/K
  • D. 44.03 J/K

Q2. For an ideal gas undergoing reversible adiabatic compression, which relationship holds?

  • A. \(P^{1-\gamma} T^\gamma = \text{constant}\)
  • B. \(PV = \text{constant}\)
  • C. \(T/V = \text{constant}\)
  • D. \(P/T = \text{constant}\)

Q3. A system at constant volume absorbs 208 J of heat, and its temperature increases from 300 K to 310 K. What is \( C_v \)? (1 mol diatomic gas)

  • A. 12.5 J/mol·K
  • B. 20.8 J/mol·K
  • C. 30.0 J/mol·K
  • D. 90.0 J/mol·K

Q4. Calculate \(\Delta H\) for \(C(s) + 2H_2O(g) \rightarrow CO_2(g) + 2H_2(g)\) using: \(\Delta H_f^\circ (H_2O,g) = -241.8 \, \text{kJ/mol}\), \(\Delta H_f^\circ (CO_2,g) = -393.5 \, \text{kJ/mol}\).

  • A. -90.1 kJ/mol
  • B. 483.6 kJ/mol
  • C. 90.1 kJ/mol
  • D. -393.5 kJ/mol

Q5. The standard enthalpy change for the reaction \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\) is given by:

  • A. \(2 \times \Delta_f H^\circ (NH_3)\)
  • B. \(\Delta_f H^\circ (N_2) + 3 \times \Delta_f H^\circ (H_2)\)
  • C. \(\Delta_f H^\circ (NH_3) - \Delta_f H^\circ (N_2)\)
  • D. \(\Delta_f H^\circ (NH_3) / 2\)

+ 5 more questions in the actual test

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