Recommended PYQs (STRICTLY NCERT Based) Thermodynamics Chemistry (2022) NEET Practice Questions, MCQs, Past Year Questions (PYQs), NCERT Questions, Question Bank, Class 11 and Class 12 Questions, and PDF solved with answers

Match List I with List II.

	List-I (Process)		List-II (Conditions)
A.	Isothermal process	I.	No heat exchange
B.	Isochoric process	II.	Carried out at constant temperature
C.	Isobaric process	III.	Carried out at constant volume
D.	Adiabatic process	IV.	Carried out at constant pressure

Choose the correct answer from the options given below:
1.

A-IV, B-II, C-III, D-I

$\text { A-IV, B-II, C-III, D-I }$
2.

A-I, B-II, C-III, D-IV

$\text { A-I, B-II, C-III, D-IV }$
3.

A-II, B-III, C-IV, D-I

$\text { A-II, B-III, C-IV, D-I }$
4.

A-IV, B-III, C-II, D-I

$\text { A-IV, B-III, C-II, D-I }$

Subtopic: Thermodynamics' Properties and process |

87%

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Q2:

In which of the following processes entropy increases?

A.	A liquid evaporates to vapour.
B.	Temperature of a crystalline solid lowered from $130~\text{K}$ to $0~\text{K}.$
C.	$2 \mathrm{NaHCO}_{3(\mathrm{~s})} \rightarrow \mathrm{Na}_2 \mathrm{CO}_{3(\mathrm{~s})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$
D.	$\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{(\mathrm{g})}$

Choose the correct answer from the options given below:

1.	$\text { A, B and D }$	2.	$\text { A, C and D }$
3.	$\text { C and D }$	4.	$\text { A and C }$

Subtopic: Spontaneity & Entropy |

75%

From NCERT

NEET - 2024

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Q3:

The work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from pressure of 20 atmosphere to 10 atmosphere is :
(Given R = 2.0 cal K^–1 mol^–1)

1. –413.14 calories
2. 413.14 calories
3. 100 calories
4. 0 calorie

Subtopic: First Law of Thermodynamics |

72%

From NCERT

NEET - 2024

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Q4:

Enthalpy of combustion of carbon to carbon dioxide is

- 390.0 {kJ mol}^{- 1} .

$-390.0~\text{kJ mol}^{-1}.$ The amount of heat released when

35.0 g

$35.0~\text{g}$ of

C O_{2}

$\mathrm{CO_2}$ is formed from the reaction of carbon and dioxygen gas, is:

1.

310 kJ

$310~\text{kJ}$
2.

490 kJ

$490~\text{kJ}$
3.

245 kJ

$245~\text{kJ}$
4.

700 kJ

$700~\text{kJ}$

Subtopic: Enthalpy & Internal energy |

76%

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Q5:

Choose the correct statement for the work done in the expansion and heat absorbed or released when 5 liters of an ideal gas at 10 atmospheric pressure isothermally expands into a vacuum until the volume is 15 liters:

1.	Both the heat and work done will be greater than zero.
2.	Heat absorbed will be less than zero and work done will be positive.
3.	Work done will be zero and heat absorbed or evolved will also be zero.
4.	Work done will be greater than zero and heat absorbed will remain zero.

Subtopic: First Law of Thermodynamics |

64%

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Q6:

For an endothermic reaction:
A.

q_{p}

$q_p$ (heat at constant pressure) is negative.
B.

Δ_{r} H

$\Delta _r H$ (enthalpy change of the reaction) is positive.
C.

Δ_{r} H

$\Delta _r H$ is negative.
D.

q_{p}

$q_p$ is positive.
Which of the following combinations is correct?

1. B and D
2. C and D
3. A and B
4. A and C

Subtopic: Thermodynamics' Properties and process |

73%

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Q7:

For the following reaction at 300K

A_{2} (g) + 3 B_{2} (g) \to 2 {A B}_{3} (g)

$\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})$
the enthalpy change is +15 kJ, then the internal energy change is:

1. 19.98 K J
2. 200 J
3. 1999 J
4. 1.9988 kJ

Subtopic: Enthalpy & Internal energy |

77%

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Q8:

What is the correct relationship between changes in enthalpy and internal energy within the following options?
1.

Δ H + Δ U = Δ n R

$\mathrm{\Delta {H}+\Delta {U}=\Delta {nR}}$
2.

Δ H = Δ U - Δ n_{g} R T

$\mathrm{\Delta {H}=\Delta {U -\Delta n_gRT}}$
3.

Δ H = Δ U + Δ n_{g} R T

$\mathrm{\Delta {H}=\Delta {U+\Delta n_gRT }}$
4.

Δ H - Δ U = - Δ n_{g} R T

$\mathrm{\Delta {H} -\Delta {U=-\Delta n_gRT}}$

Subtopic: Enthalpy & Internal energy |

83%

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Q9:

Consider the following reaction:

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (g) Δ_{r} H^{\circ} = - 483.64 k J .

$\mathrm{2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \Delta_rH^\circ = -483.64 kJ. }$
What is the enthalpy change for the decomposition of one mole of water?

1.	120.9 kJ	2.	241.82 kJ
3.	18 kJ	4.	100 kJ

Subtopic: Thermochemistry |

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Q10:

Which p-V curve among the following depicts the highest amount of work done?

1.		2.
3.		4.

Subtopic: 2nd & 3rd Law of Thermodynamics |

86%

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