Q. No.Consider the following graph.
The work done, as per the graph above, is:
1.
Positive
2.
Negative
3.
Zero
4.
Cannot be determined
Consider the following diagram for a reaction .
The nature of the reaction is-
1. Exothermic
2. Endothermic
3. Reaction at equilibrium
4. None of the above
What is the nature of the reaction depicted in the given diagram for A→C?
| 1. | Exothermic | 2. | Endothermic |
| 3. | Reaction at equilibrium | 4. | None of these |
An enthalpy diagram for a particular reaction is given below:
Which of the following statements is correct?
| 1. | Reaction is spontaneous |
| 2. | Reaction is non-spontaneous |
| 3. | The spontaneity of the reaction cannot be determined from the graph provided above. |
| 4. | None of the above |
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 |
| (i) | When liquid crystallizes into a solid, entropy increases. |
| (ii) | When the temperature of a crystalline solid is raised from 0 K to 115 K then entropy increases. |
| (iii) | 2 NaHCO3 (s) →Na2CO3 (s) +CO2(g)+H2O(g); Entropy increases. |
| (iv) | H2(g)→2H(g) ; Entropy decreases. |
For one mole of an ideal gas, which of these statements must be true?
(I) U and H each depend only on temperature.
(II) Compressibility factor z is not equal to 1.
(III) CP, m – CV, m = R
(IV) dU = CVdT for any process.
1. (I), (III) and (IV)
2. (II), (III) and (IV)
3. (III) and (IV)
4. (I) and (III)
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 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
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