Q. No.Select the correct option based on statements below:
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.
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| 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. |
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| Assertion (A): | Specific heat is an intensive property. |
| Reason (R): | Heat capacity 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. |
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The thermodynamic stability of NO(g) based on the above data is:
1. Less than NO2(g)
2. More than NO2(g)
3. Equal to NO2(g)
4. Insufficient data
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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 |
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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
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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 |
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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 |
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. The standard enthalpy of formation of gas in the above reaction would be-
| 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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