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 |
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| (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
| 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, \(\Delta H = q_p \) |
Five moles of an ideal gas at 1 bar and 298 K undergo free expansion (expansion into vacuum) such that its volume becomes double. Calculate the work done during the process:
2. \( \text {-RT }\left(\mathrm{V}_2-\mathrm{V}_1\right) \)
3. \( \text {-RT } \ln \mathrm({V}_1 / \mathrm{V}_2 )\)
4. Zero
1. 20 \(\mathrm{L}\) atm
2. 0 \(\mathrm{L}\) atm
3. 40 \(\mathrm{L}\) atm
4. 24 \(\mathrm{L}\) atm
| 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
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
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One mole of a monoatomic ideal gas is expanded against a constant external pressure of 2 atm from an initial volume of 10 L to a final volume of 60 L at a constant temperature of 27°C.
Calculate the work done (in L·atm) for the above expansion process:
1. –10 L-atm2. –100 L-atm
3. –200 L-atm
4. –400 L-atm
| 1. | 8000 J | 2. | 2000 J |
| 3. | 6000 J | 4. | 7600 J |
An ideal gas undergoes isothermal expansion from 4 L to 20 L against vacuum.
Calculate the amount of heat absorbed during the process:
2. –50 kJ
3. 50 kJ
4. –40 kJ
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