Select Chapter Topics:
Q. No.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 |
56%
Level 3: 35%-60%
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
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 |
73%
Level 2: 60%+
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
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 |
52%
Level 3: 35%-60%
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
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
Please attempt this question first.
Hints
Please attempt this question first.
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
Please attempt this question first.
Hints
Please attempt this question first.
Find the amount of heat released when 35.0 g of CO₂ is formed from the combustion of carbon in dioxygen gas. Given that the enthalpy of combustion of carbon to carbon dioxide is −390.0 kJ mol⁻¹.
| 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
Hints
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
Hints
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
Hints
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
Hints
Select Chapter Topics:
© 2026 GoodEd Technologies Pvt. Ltd.