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 |
| Statement I: | Total enthalpy change of a multistep process is the sum of ∆H1 + ∆H2 + ∆H3 + . . . |
| Statement II: | When heat is absorbed by the system, the sign of q is taken to be negative. |
| 1. | Statement I is correct; Statement II is correct. |
| 2. | Statement I is correct; Statement II is incorrect. |
| 3. | Statement I is incorrect; Statement II is correct. |
| 4. | Statement I is incorrect; Statement II is incorrect. |
| Assertion (A): | Work done in an irreversible isothermal process at constant volume is zero. |
| Reason (R): | Work is assigned a negative sign during expansion and is assigned a positive sign during compression. |
| 1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
| 3. | (A) is true but (R) is false. |
| 4. | Both (A) and (R) are false. |
A sample containing 1.0 mol of an ideal gas undergoes an isothermal, reversible expansion to ten times its original volume in two separate experiments. The expansion is carried out at temperatures of 300 K and 600 K, respectively.
The correct statements among the following are:
| (a) | Work done at 600 K is 20 times the work done at 300 K. |
| (b) | Work done at 300 K is twice the work done at 600 K. |
| (c) | Work done at 600 K is twice the work done at 300 K. |
| (d) | ∆ U = 0 in both cases. |
1. (a) and (b)
2. (b) and (c)
3. (c) and (d)
4. (a) and (d)
Consider the given reaction"
\(2 Zn(s) + O_2 (g) \rightarrow 2ZnO(s)\)
For this reaction, \(\Delta H = -693.8~ \text {kJ mol}^{-1}\).
The correct statements among the following are :
| a. | The enthalpy of two moles of ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ. |
| b. | The enthalpy of two moles of ZnO is more than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ. |
| c. | 693 . 8 kJ mol -1 energy is evolved in the reaction. |
| d. | 693 . 8 kJ mol -1 energy is absorbed in the reaction. |
1. a and b
2. b and c
3. c and d
4. a and c
For the graph given below, it can be concluded that work done during the process shown will be-
| 1. | Zero | 2. | Negative |
| 3. | Positive | 4. | Cannot be determined |
Consider the following graph.
The work done, as per the graph above, is:
| 1. | Positive | 2. | Negative |
| 3. | Zero | 4. | Cannot be determined |
1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in the graph below:
The work done for the expansion of gas from state (1) to state (2) at 298 K will be:
1. 1617.6 J
2. -1617.6 J
3. 1717.6 J
4. -1717.6 J
| Column-I (Process) |
Column-II (Expression)
|
||
| a. | No heat is absorbed by the system from the surroundings, but work (w) is done on the system. | i. | ∆U = q – w, closed system. |
| b. | No work is done on the system, but q amount of heat is taken out from the system and given to the surroundings. | ii. | ΔU=Wad, for an adiabatic wall. |
| c. | w amount of work is done by the system and q amount of heat is supplied to the system. | iii. | ∆U = –q, thermally conducting walls. |
| 1. | a = i; b = ii; c = iii | 2. | a = ii; b = i; c = iii |
| 3. | a = ii; b = iii; c = i | 4. | a = iii; b = ii; c = i |
| Assertion (A): | \(C_p - C_v = R \), for 1 mole of an ideal gas. |
| Reason (R): | R is equal to the work done when the temperature of one mole of an ideal gas is increased by 1º. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | Both (A) and (R) are False. |
© 2025 GoodEd Technologies Pvt. Ltd.