Q. No.| Assertion (A): | Variables like P, V, and T are called state functions. |
| Reason (R): |
Their values depend solely on the system's state, and not on how it is reached. |
| 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. |
| Assertion (A): | Pressure is an intensive property. |
| Reason (R): | Volume is an extensive property. |
| 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. |
| Reaction | Δ Hºrxn, kJ mol–1 |
| H2S + 1.5O2 → SO2 + H2O | –518.2 |
| 2H2S + CO2 → CS2 + 2H2O | 67.8 |
| CS2 + 3O2 → CO2 + 2SO2 | ??? |
2. –586.0 kJ mol–1
3. –968.6 kJ mol–1
4. –1104.2 kJ mol–1
1. 157 kJ mol-1
2. –1574 kJ mol-1
3. –394 kJ mol-1
4. 32.8 kJ mol-1
1. Ca(s) + \(\frac{1}{8}\) S8(s, rhombic) + \(\frac{3}{2}\) O2(g) → CaSO3(s)
2. 8Ca(s) + S8(s) + 12O2(g) → 8CaSO3(s)
3. 8Ca(s) + S8(g) + 12O2(g) → 8CaSO3(s)
4. CaO(s) + SO2(g) → CaSO3(s)
Calculate the Gibbs energy change when 1 mole of NaCl is dissolved in water at 298 K. Given,
a. Lattice energy of NaCl = 778 kJ mol-1
b. Hydration energy of NaCl =-774.3 kJ mol-1
c. Entropy change at 298 K = 43 JK-1 mol-1
| 1. | -3.7 kJ | 2. | -9.1 kJ |
| 3. | -43 kJ | 4. | -13.14 kJ |
Which of the following reactions has the least difference between the change in enthalpy (∆H) and the change in internal energy (∆E) at a given temperature?
1. \(2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{SO}_3(\mathrm{~g})\)
2. \(\mathrm{CaCO}_3(s) \rightarrow \mathrm{CaO}(s)+\mathrm{CO}_2(g)\)
3. \(\mathrm{NH}_4 \mathrm{SH} (s) ~~\rightarrow ~\mathrm{NH}_3(g)+\mathrm{H}_2 \mathrm{~S}(g)\)
4. \(2 \mathrm{NH}_3 (g) ~\rightarrow ~\mathrm{N}_2(g)+3 \mathrm{H}_2(g)\)
A system that can neither exchange matter nor energy with the surroundings is classified as:
1. Open system
2. Isolated system
3. Closed system
4. Both (1) & (2)
The standard enthalpies of the formation of NO2(g) and N2O4(g) are 8 kcal mol–1 and 2 kcal mol–1 respectively. The heat of dimerization of NO2 in the gaseous state is:
| 1. | 10 k cal mol–1 | 2. | 6.0 k cal mol–1 |
| 3. | –14 k cal mol–1 | 4. | –6.0 k cal mol–1 |
1. H > 0 and S< 0
2. H < 0 and S> 0
3. H < 0 and S< 0
4. H > 0 and S = 0
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