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Q. No.In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?
| 1. | \(2\mathrm{SO}_2(g)+\mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{SO}_3(g)\) |
| 2. | \(\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \rightleftharpoons 2 \mathrm{NH}_3(g)\) |
| 3. | \(\mathrm{NO}_2(g)+\mathrm{SO}_2(g) \rightleftharpoons \mathrm{SO}_3(g)+\mathrm{NO}(g)\) |
| 4. | \(\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)\) |
Subtopic: Le Chatelier's principle |
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Level 1: 80%+
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Match List-I with List-II:
| List-I | List-II | ||
|---|---|---|---|
| (A) | Le Chatelier's principle | (i) | Suppresses the solubility of AgCl |
| (B) | Common ion effect | (ii) | Resists change in pH |
| (C) | Buffer solution | (iii) | Shifts the equilibrium to the side with fewer gas molecules |
| (D) | Increase in pressure | (iv) | Predicts the direction of shift on adding stress |
Choose the most appropriate answer from the options given below:
1. (A)–(iv), (B)–(i), (C)–(ii), (D)–(iii)
2. (A)–(i), (B)–(ii), (C)–(iii), (D)–(iv)
3. (A)–(iv), (B)–(iii), (C)–(i), (D)–(ii)
4. (A)–(ii), (B)–(i), (C)–(iv), (D)–(iii)
Subtopic: Introduction To Equilibrium | Le Chatelier's principle |
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The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal.
\(\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{l})+3 \mathrm{CO}_2(\mathrm{~g})\)
Using Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium:
\(\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{l})+3 \mathrm{CO}_2(\mathrm{~g})\)
Using Le Chatelier’s principle, predict which one of the following will not disturb the equilibrium:
| 1. | \(\text {Removal of} ~\mathrm{CO} \) | 2. | \(\text {Removal of} ~\mathrm{CO_2}\) |
| 3. | \(\text {Addition of} ~\mathrm{CO_2}\) | 4. | \(\text {Addition of} ~\mathrm{Fe_2O_3}\) |
Subtopic: Le Chatelier's principle |
87%
Level 1: 80%+
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For the reversible reaction \(N_2(g)+3H_2(g)⇌2NH_3(g)\), what is the effect on the equilibrium position when an inert gas is added at constant volume?
| 1. | Shifts in the forward reaction |
| 2. | Shifts in backward reaction |
| 3. | Remains unaffected |
| 4. | Initially in the forward direction and then in the backward direction |
Subtopic: Le Chatelier's principle |
86%
Level 1: 80%+
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Find the condition that shifts the following exothermic equilibrium towards the formation of NH₃:
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heat
1. Increasing the concentration of NH₃2. Decreasing the pressure
3. Decreasing the concentration of H₂
4. Increasing the pressure and decreasing the temperature
Subtopic: Le Chatelier's principle |
86%
Level 1: 80%+
AIPMT - 2014
Hints
In which cases will the reaction proceed towards the right side on increasing the pressure?
1. (a) and (c)
2. (a) and (b)
3. (c) and (d)
4. None of the above
| (a) | \(4 \mathrm{HCl}(g)+\mathrm{O}_2(g) \longrightarrow 2 \mathrm{Cl}_2(g)+2 \mathrm{H}_2 \mathrm{O}(g)\) |
| (b) | \(\mathrm{Cl}_2(g)+\mathrm{H}_2 \mathrm{O}(g) \longrightarrow 2 \mathrm{HCl}(g)+\frac{1}{2} \mathrm{O}_2(g) \) |
| (c) | \(\mathrm{CO}_2(\mathrm{~g})+4 \mathrm{H}_2(\mathrm{~g}) \longrightarrow \mathrm{CH}_4(\mathrm{~g})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) \) |
| (d) | \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}(\mathrm{g})\) |
1. (a) and (c)
2. (a) and (b)
3. (c) and (d)
4. None of the above
Subtopic: Le Chatelier's principle |
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Level 1: 80%+
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