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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 |
74%
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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Level 3: 35%-60%
NEET - 2026
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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 |
86%
Level 1: 80%+
NEET - 2024
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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 |
73%
Level 2: 60%+
NEET - 2024
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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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Enthalpy of combustion of carbon to carbon dioxide is \(-390.0~\text{kJ mol}^{-1}.\) The amount of heat released when \(35.0~\text{g}\) of \(\mathrm{CO_2}\) is formed from the reaction of carbon and dioxygen gas, is:
| 1. | \(310~\text{kJ}\) | 2. | \(490~\text{kJ}\) |
| 3. | \(245~\text{kJ}\) | 4. | \(700~\text{kJ}\) |
Subtopic: Enthalpy & Internal energy |
74%
Level 2: 60%+
NEET - 2024
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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 |
62%
Level 2: 60%+
NEET - 2024
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For an endothermic reaction:
A. \(q_p \) (heat at constant pressure) is negative.
B. \(\Delta _r H \) (enthalpy change of the reaction) is positive.
C. \(\Delta _r H \) is negative.
D. \(q_p \) is positive.
Which of the following combinations is correct?
A. \(q_p \) (heat at constant pressure) is negative.
B. \(\Delta _r H \) (enthalpy change of the reaction) is positive.
C. \(\Delta _r H \) is negative.
D. \(q_p \) 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%
Level 2: 60%+
NEET - 2024
Hints
Consider the following reaction:
\(\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})\)
If at 300K, the enthalpy change for the above reaction is +15 kJ, then the internal energy change is:
\(\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})\)
If at 300K, the enthalpy change for the above reaction 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 |
76%
Level 2: 60%+
NEET - 2024
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