Q. No.Match the terms in List I with their corresponding descriptions in List II:
| List I (Term) | List II (Description) | ||
| A. | Adiabatic process | i. | At constant temperature |
| B. | Isolated system | ii. | No transfer of heat |
| C. | Isothermal change | iii. | Heat |
| D. | Path function | iv. | No exchange of energy and matter |
Codes:
| A | B | C | D | |
| 1. | ii | iv | i | iii |
| 2. | iii | iv | i | ii |
| 3. | iv | iii | i | ii |
| 4. | iv | ii | i | iii |
Subtopic: First Law of Thermodynamics | Classification of System, Extensive & Intensive Properties |
85%
Level 1: 80%+
Hints
Which of the following statements is/are correct?
1. a and b
2. b, c and d
3. b and c
4. None of the above
| (a) | Heat is a way of transferring energy. |
| (b) | Heat is not a property of the system, whereas temperature is a property of the system. |
| (c) | Reactions that are accompanied by the evolution of heat are called endothermic reactions. |
| (d) | Those reactions in which heat is absorbed are known as exothermic reactions. |
1. a and b
2. b, c and d
3. b and c
4. None of the above
Subtopic: First Law of Thermodynamics | Classification of System, Extensive & Intensive Properties | Thermochemistry |
84%
Level 1: 80%+
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Choose the incorrect statement from the following :
| 1. | In a reversible process, the system and surroundings are always in equilibrium with each other. |
| 2. | Work done in free expansion > 0. |
| 3. | For adiabatic change, \(\Delta q \) = 0 . |
| 4. | For a process carried at constant pressure, \(\Delta H = q_p \) |
Subtopic: First Law of Thermodynamics | Enthalpy & Internal energy |
86%
Level 1: 80%+
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Five moles of an ideal gas at 1 bar and 298 K is expanded into vacuum to double the volume. The work done is:
1. \( \mathrm{C}_{\mathrm{V}}\left(\mathrm{T}_2-\mathrm{T}_1\right)\)
2. \( \text {-RT }\left(\mathrm{V}_2-\mathrm{V}_1\right) \)
3. \( \text {-RT } \ln \mathrm({V}_1 / \mathrm{V}_2 )\)
4. Zero
1. \( \mathrm{C}_{\mathrm{V}}\left(\mathrm{T}_2-\mathrm{T}_1\right)\)
2. \( \text {-RT }\left(\mathrm{V}_2-\mathrm{V}_1\right) \)
3. \( \text {-RT } \ln \mathrm({V}_1 / \mathrm{V}_2 )\)
4. Zero
Subtopic: First Law of Thermodynamics | Enthalpy & Internal energy |
86%
Level 1: 80%+
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What is the amount of heat absorbed in the expansion of an ideal gas from \(\mathrm{4.0 ~L}\) to \(\mathrm{20~ L}\) when the gas is allowed to expand isothermally into a vacuum:
1. 20 \(\mathrm{L}\) atm
2. 0 \(\mathrm{L}\) atm
3. 40 \(\mathrm{L}\) atm
4. 24 \(\mathrm{L}\) atm
1. 20 \(\mathrm{L}\) atm
2. 0 \(\mathrm{L}\) atm
3. 40 \(\mathrm{L}\) atm
4. 24 \(\mathrm{L}\) atm
Subtopic: First Law of Thermodynamics |
95%
Level 1: 80%+
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The correct match for the following options is:
1. A → Q, B → P, C → S, D → R
2. A → P, B → Q, C → R, D → S
3. A → S, B → R, C → Q, D → P
4. A → P, B → R, C → S, D → Q
| List I | List II | ||
| (A) | Adiabatic | (P) | ∆T = 0 |
| (B) | Isothermal | (Q) | Heat exchange is zero |
| (C) | Isochoric | (R) | ∆P = 0 |
| (D) | Isobaric | (S) | Work done is zero |
1. A → Q, B → P, C → S, D → R
2. A → P, B → Q, C → R, D → S
3. A → S, B → R, C → Q, D → P
4. A → P, B → R, C → S, D → Q
Subtopic: First Law of Thermodynamics |
93%
Level 1: 80%+
JEE
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Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be:
1. 3 Joules
2. 9 Joules
3. Zero
4. Infinite
Subtopic: First Law of Thermodynamics |
92%
Level 1: 80%+
AIPMT - 2010
Hints
1 mol monoatomic ideal gas expanded against 2 atm pressure from 10 L to 60 L at 27°C. Work done in above process is
1. –10 L-atm
2. –100 L-atm
3. –200 L-atm
4. –400 L-atm
1. –10 L-atm
2. –100 L-atm
3. –200 L-atm
4. –400 L-atm
Subtopic: First Law of Thermodynamics |
91%
Level 1: 80%+
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Calculate the magnitude of heat (q) in joules for an isothermal irreversible expansion, where the system expands against an external pressure of 8 bar, and the volume increases by 10 L.
| 1. | 8000 J | 2. | 2000 J |
| 3. | 6000 J | 4. | 7600 J |
Subtopic: First Law of Thermodynamics |
89%
Level 1: 80%+
JEE
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Calculate the amount of heat is absorbed for an ideal gas which expands isothermally from 4 litre to 20 litre against the vacuum.
1. 0
2. –50 kJ
3. 50 kJ
4. –40 kJ
1. 0
2. –50 kJ
3. 50 kJ
4. –40 kJ
Subtopic: First Law of Thermodynamics |
88%
Level 1: 80%+
JEE
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