NEET Chemistry: Thermodynamics — MCQ Test 11

Q6. For which process is \(\Delta H = \Delta U\)?

Q7. Calculate the heat absorbed when 27 g of aluminum is heated from 25°C to 125°C at constant volume. (\(C_v = 22.4 \, \text{J/mol·K}\), molar mass = 27 g/mol)

Q8. Calculate \(\Delta G^\circ\) for a reaction with \(K = 1.5 \times 10^{-4}\) at 298 K. (\(R = 8.314 \, \text{J/mol·K}\))

Q9. For a reaction with \(K = 0.01\) at 298 K, calculate \(\Delta G^\circ\). (\(R = 8.314 \, \text{J/mol·K}\))

Q10. For an adiabatic process, which condition must be satisfied?

NEET Chemistry — Thermodynamics

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For H2O(l)→H2(g)+12O2(g)H_2O(l) \rightarrow H_2(g) + \frac{1}{2}O_2(g), ΔH=285.80 kJ/mol\Delta H = 285.80 \, \text{kJ/mol} at 298 K. What is ΔU\Delta U? (R=8.314 J/mol\cdotpKR = 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 Rightarrow, Expanding, Adiabatically, Temperature, Reaction, and Calculate.

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.

For H2O(l)→H2(g)+12O2(g)H_2O(l) \rightarrow H_2(g) + \frac{1}{2}O_2(g), ΔH=285.80 kJ/mol\Delta H = 285.80 \, \text{kJ/mol} at 298 K. What is ΔU\Delta U? (R=8.314 J/mol\cdotpKR = 8.314 \, \text{J/mol·K})

  • A.

    285.8 kJ/mol

  • B.

    282.1 kJ/mol

  • C.

    289.5 kJ/mol

  • D.

    279.3 kJ/mol

Q2.

For an ideal gas (γ=1.5\gamma = 1.5) expanding adiabatically from 10 L to 25 L at 600 K, what is the final temperature?

  • A.

    240 K

  • B.

    379.2 K

  • C.

    948 K

  • D.

    600 K

Q3.

For a reaction with ΔH=−80.00 kJ/mol\Delta H = -80.00 \, \text{kJ/mol} and ΔS=−200.0 J/K\cdotpmol\Delta S = -200.0 \, \text{J/K·mol} , what is ΔG\Delta G at 300 K?

  • A.

    80 kJ/mol

  • B.

    -60 kJ/mol

  • C.

    20 kJ/mol

  • D.

    -20 kJ/mol

Q4.

For the process 2NO2(g)→N2O4(g)2NO_2(g) \rightarrow N_2O_4(g), ΔH=−57.20 kJ/mol\Delta H = -57.20 \, \text{kJ/mol} at 298 K, what is ΔU\Delta U? (R=8.314 J/mol\cdotpKR = 8.314 \, \text{J/mol·K})

  • A.

    -59.68 kJ/mol

  • B.

    -57.2 kJ/mol

  • C.

    -52.24 kJ/mol

  • D.

    -54.72 kJ/mol

Q5.

Calculate ΔS\Delta S for the fusion of 36 g of ice at 273 K if ΔHfus=6.01 kJ/mol\Delta H_{fus} = 6.01 \, \text{kJ/mol}. (Molar mass of H2O=18 g/molH_2O = 18 \, \text{g/mol})

  • A.

    22 J/K

  • B.

    6.01 J/K

  • C.

    44 J/K

  • D.

    88 J/K

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