Q. No.Select the correct option based on the statements given below:
Statement I.
Specific heat is an intensive property.
Statement II.
Heat capacity is an extensive property.
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): | Dissolution of sugar in water proceeds via an increase in entropy. |
| Reason (R): | Entropy decreases, when an egg is boiled hard. |
| 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): | 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. |
1. Less than NO2(g)
2. More than NO2(g)
3. Equal to NO2(g)
4. Insufficient data
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 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 |
Determine the value of ∆G°, if the equilibrium constant for a reaction is 10:
( )
1. \(-5.74 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
2. \(-5.74 \mathrm{~J} \mathrm{~mol}^{-1}\)
3. \( +4.57 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. \(-57.4 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
The standard enthalpy of the formation of CH3OH(l) from the following data is:
| \(\small{\mathrm{CH}_3 \mathrm{OH}_{(l)}+\frac{3}{2} \mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{CO}_2(\mathrm{g})+2 \mathrm{H}_2 \mathrm{O}_{(l)} \text {; }}\) \( \Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-726 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}\) |
| \(\small{\mathrm{C}(\mathrm{s})+\mathrm{O}_2(\mathrm{g}) \rightarrow \mathrm{CO}_2(\mathrm{g}) \text {; } }\) \(\Delta_{\mathrm{c}} \mathrm{H}^{\circ}=-393 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}\) |
| \(\small{\mathrm{H}_{2(\mathrm{g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{g})} \rightarrow \mathrm{H}_2 \mathrm{O}_{(l)} \text {; } } \) \(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}\) |
| 1. | −239 kJ mol−1 | 2. | +239 kJ mol−1 |
| 3. | −47 kJ mol−1 | 4. | +47 kJ mol−1 |
For the reaction:
N₂(g) + 3H₂(g) → 2NH₃(g) ; ΔᵣH° = –92.4 kJ mol⁻¹
What is the standard enthalpy of formation (ΔfH°) of NH₃(g)?
| 1. | -92.4 J (mol)-1 | 2. | -46.2 kJ (mol)-1 |
| 3. | +46.2 J (mol)-1 | 4. | +92.4 kJ (mol)-1 |
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