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Q. No.At a certain temperature, T(K), during a process, 500 J is absorbed by the system and work of 200 J is done by the system. Then change in internal energy of the system is :
1. 700 J
2. 300 J
3. 400 J
4. 500 J
1. 700 J
2. 300 J
3. 400 J
4. 500 J
Subtopic: First Law of Thermodynamics |
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Level 2: 60%+
NEET - 2026
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Consider the following reaction:
2A (g) + B (g) → 2D (g)
\(ΔU^⊖\)=−10 \(kJ mol^{−1}\) and \(ΔS^⊖\)=−44 \(J K^{−1}\) at 298 K.
Identify the correct option with \(ΔG^⊖\) for the reaction and spontaneity of the reaction at 298 K.
(Given : R=\(8.31 ~J mol^{−1} K^{−1}\))
2A (g) + B (g) → 2D (g)
\(ΔU^⊖\)=−10 \(kJ mol^{−1}\) and \(ΔS^⊖\)=−44 \(J K^{−1}\) at 298 K.
Identify the correct option with \(ΔG^⊖\) for the reaction and spontaneity of the reaction at 298 K.
(Given : R=\(8.31 ~J mol^{−1} K^{−1}\))
| 1. | −1.635 kJ mol−1, spontaneous |
| 2. | +0.63568 kJ mol−1, non-spontaneous |
| 3. | −0.63568 kJ mol−1, spontaneous |
| 4. | +1.635 kJ mol−1, non-spontaneous |
Subtopic: Spontaneity & Entropy | Gibbs Energy Change |
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Two moles of an ideal gas undergo free expansion from 10 L to 100 L at 300 K. The Values of \(\Delta \mathrm{S}_{\text {system }}\) and \(\Delta \mathrm{S}_{\text {surroundings }}\) are :
(R is universal gas constant)
(R is universal gas constant)
| 1. | \(\Delta \mathrm{S}_{\text {system }}=4.606 \mathrm~{R} ; \Delta \mathrm{S}_{\text {surroundings }}=0\) |
| 2. | \(\Delta \mathrm{~S}_{\text {system }}=0 ;~ \Delta \mathrm{S}_{\text {surroundings }}=0 \) |
| 3. | \(\Delta \mathrm{~S}_{\text {system }}=4.606~ \mathrm{R} ; \Delta \mathrm{S}_{\text {surroundings }}= -4.606 \mathrm{R}\) |
| 4. | \(\Delta \mathrm{~S}_{\text {system }}=0 ; \quad \Delta ~~\mathrm{S}_{\text {surroundings }}= 4.606 \mathrm{R}\) |
Subtopic: Spontaneity & Entropy |
Level 4: Below 35%
NEET - 2026
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Consider the reversible processes for 1.0 mol of an ideal gas as shown in the figure.
w₁, w₂, w₃ and w₄ represent work done (in calories) in the processes 1, 2, 3 and 4, respectively; ΔU₂ and ΔU₄ are changes in the internal energy for the processes 2 and 4, respectively. [use R = 2 cal K⁻¹ mol⁻¹]
The correct option is:
w₁, w₂, w₃ and w₄ represent work done (in calories) in the processes 1, 2, 3 and 4, respectively; ΔU₂ and ΔU₄ are changes in the internal energy for the processes 2 and 4, respectively. [use R = 2 cal K⁻¹ mol⁻¹]
The correct option is:
| 1. | w₁ + w₂ + w₃ + w₄ = 0 |
| 2. | w₁ + w₃ = -2T₁ ln \(\frac{V₂}{V₁}\) - 2T₂ ln \(\frac{V₄}{V₃}\) |
| 3. | w₂ + w₄ = ΔU₂ - ΔU₄ |
| 4. | w₁ + w₂ = 2T₁ ln \(\frac{V₂}{V₁}\) |
Subtopic: Thermodynamics' Properties and process |
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The standard heat of formation, in kcal/mol of \(Ba^{2+}\) is :
[Given : standard heat of formation of \(SO^{2-}_4\) ion (aq) \(= -216~ \text{kcal/mol}\), standard heat of crystallisation of \(BaSO_4 (s)= -4.5~\text{ kcal/mol,}\) standard heat of formation of \(BaSO_4 (s)= -349 ~\text{kcal/mol]}\)
[Given : standard heat of formation of \(SO^{2-}_4\) ion (aq) \(= -216~ \text{kcal/mol}\), standard heat of crystallisation of \(BaSO_4 (s)= -4.5~\text{ kcal/mol,}\) standard heat of formation of \(BaSO_4 (s)= -349 ~\text{kcal/mol]}\)
| 1. | \(+133.0 \) | 2. | \(+220.5\) |
| 3. | \(-128.5 \) | 4. | \(-133.0\) |
Subtopic: Thermochemistry |
Level 3: 35%-60%
NEET - 2025
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Match List I with List II.
Choose the correct answer from the options given below:
| 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 |
| 1. | \(\text { A-IV, B-II, C-III, D-I }\) | 2. | \(\text { A-I, B-II, C-III, D-IV }\) |
| 3. | \(\text { A-II, B-III, C-IV, D-I }\) | 4. | \(\text { A-IV, B-III, C-II, D-I }\) |
Subtopic: Thermodynamics' Properties and process |
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In which of the following processes entropy increases?
Choose the correct answer from the options given below:
| 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. | \(\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{(\mathrm{g})}\) |
| 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 |
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Work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from a pressure of 20 atmospheres to a pressure of 10 atmospheres is:
(Given: R = 2.0 cal K–1 mol–1)
(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 |
70%
Level 2: 60%+
NEET - 2024
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If the standard enthalpy of neutralization reaction of \(\text{HCl }\) and \(\mathrm{NaOH}\) is \(-57.3 \mathrm{~K}{\mathrm{J}}~ \mathrm{mol}^{-1}\), then find out the enthalpy of neutralization of \(0.25 \mathrm{~mol}\) of \(\text{HCl }\)by \(0.25 \mathrm{~mol}\) of \(\mathrm{NaOH}\) :
1. \(-57.3~ \mathrm{kJ} ~\mathrm{mol}^{-1}\)
2. \(-28.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3. \(-14.32 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. \(+57.3~ \mathrm{kJ}~ \mathrm{mol}^{-1}\)
1. \(-57.3~ \mathrm{kJ} ~\mathrm{mol}^{-1}\)
2. \(-28.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3. \(-14.32 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. \(+57.3~ \mathrm{kJ}~ \mathrm{mol}^{-1}\)
Subtopic: Thermochemistry |
61%
Level 2: 60%+
NEET - 2024
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Match the processes or properties in List-I with their corresponding characteristics in List-II.
Choose the correct answer from the options given below:
| List-I (Process/Property) |
List-II (Characteristic) |
||
| A. | Adiabatic process | I. | Independent of the amount of substance |
| B. | Reversible process | II. | The reaction can proceed in both directions, from reactants to products and vice versa |
| C. | Intensive property | III. | No transfer of heat between the system and the surrounding |
| D. | Extensive property | IV. | Dependent on the amount of substance |
| 1. | A-II, B-III, C-IV, D-I | 2. | A-I, B-II, C-IV, D-III |
| 3. | A-III, B-II, C-I, D-IV | 4. | A-I, B-II, C-III, D-IV |
Subtopic: Classification of System, Extensive & Intensive Properties |
92%
Level 1: 80%+
NEET - 2024
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