Q. No.When will the system be identified as being in equilibrium for the chemical reaction \(A \rightleftharpoons B \)?
1. A completely changes to B.
2. 50 % of A changes to B.
3. The rate of change of A to B and B to A are the same.
4. Only 10 % of A changes to B.
1. A completely changes to B.
2. 50 % of A changes to B.
3. The rate of change of A to B and B to A are the same.
4. Only 10 % of A changes to B.
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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Match Column-I with Column-II and mark the appropriate option:
| Column-I (Term) | Column-II (Conditions) | ||
| (A) | Solute (s) ⇌ Solute (solution) | (I) | ∆G>0, K<1 |
| (B) | Spontaneous reaction | (II) | Saturated solution |
| (C) | Non-spontaneous reaction | (III) | ∆G<0, K>1 |
| (D) | Liquid ⇌ Vapour | (IV) | Boiling point |
Codes:
| A | B | C | D | |
| 1. | II | III | I | IV |
| 2. | IV | II | III | I |
| 3. | I | IV | III | II |
| 4. | II | IV | I | III |
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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The relation between the equilibrium constants \(K_1 ~\text{and}~K_2\) for the following reactions is as:
\(\begin{aligned} & \mathrm{NO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \stackrel{\mathrm{K}_1}{\rightleftharpoons} \mathrm{NO}_2(\mathrm{~g}) \text { and } \\ & 2 \mathrm{NO}_2(\mathrm{~g}) \stackrel{\mathrm{K}_2}{\rightleftharpoons} 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \end{aligned}\)
1. \(K_2={1 \over K_1}\)
2. \(K_2={K_1 \over 2}\)
3. \(K_2={1 \over K_1^2}\)
4. \(K_2=K^2_1\)
\(\begin{aligned} & \mathrm{NO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \stackrel{\mathrm{K}_1}{\rightleftharpoons} \mathrm{NO}_2(\mathrm{~g}) \text { and } \\ & 2 \mathrm{NO}_2(\mathrm{~g}) \stackrel{\mathrm{K}_2}{\rightleftharpoons} 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \end{aligned}\)
1. \(K_2={1 \over K_1}\)
2. \(K_2={K_1 \over 2}\)
3. \(K_2={1 \over K_1^2}\)
4. \(K_2=K^2_1\)
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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Choose the true statement for the equilibrium constant, Keq of a specific reaction.
1. The addition of a catalyst may change it.
2. It increases if the concentration of one of the products is increased.
3. It changes with changes in the temperature.
4. It increases if the concentration of one of the reactants is increased.
1. The addition of a catalyst may change it.
2. It increases if the concentration of one of the products is increased.
3. It changes with changes in the temperature.
4. It increases if the concentration of one of the reactants is increased.
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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Match the following equilibria with the corresponding condition.
| Column-I (Process) | Column-II (Corresponding term) |
||
| A. | Liquid ⇌ Vapour | I. | Saturated solution |
| B. | Solid ⇌ Liquid | II. | Boiling point |
| C. | Solid ⇌ Vapour | III. | Sublimation point |
| D. | Solute (s) ⇌ Solute (solution) | IV. | Melting point |
| V. | Unsaturated solution |
Codes:
| A | B | C | D | |
| 1. | II | IV | III | I |
| 2. | III | I | IV | II |
| 3. | V | IV | III | II |
| 4. | IV | V | III | II |
Subtopic: Introduction To Equilibrium |
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Given that the equilibrium constant (KC) at 800 K for the reaction N2(𝑔)+3H2(𝑔)⇋2NH3(𝑔) is 64. What is the equilibrium constant KC at the same temperature for the reaction NH3(g) ⇌ 1/2N2(g) + 3/2H2(g)?
| 1. | \(\dfrac{1}{4}\) | 2. | \(\dfrac{1}{8}\) |
| 3. | 8 | 4. | \(\dfrac{1}{64}\) |
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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| Assertion (A): | \(Ni(s)+4CO(g)\rightleftharpoons Ni(CO)_4(g)\\ \text{For the above reaction,}\\ K_C=\frac{[Ni(CO)_4]}{[CO]^4}\) |
| Reason (R): | For heterogeneous equilibrium, the concentrations of pure solids or liquids are not considered in the expression of the equilibrium constant. |
| 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. |
Subtopic: Introduction To Equilibrium |
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For the reaction equilibrium, \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_2(g) \), the concentrations of N2O4 and NO2 at equilibrium are 4.8 \(\times\) 10-2 and 1.2 \(\times\) 10-2 mol L-1 respectively. The value of Kc for the reaction is:
1. 3.3 \(\times\) 102 mol L-1
2. 3 \(\times\) 10-1 mol L-1
3. 3 \(\times\) 10-3 mol L-1
4. 3 \(\times\) 103 mol L-1
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
JEE
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The equilibrium constant for the reaction, N2(g) + O2(g) ⇌ 2NO(g) is
4 × 10–4 at 2000 K. In the presence of a catalyst,
the equilibrium is attained ten times faster.
Therefore, the equilibrium constant, in the presence of the catalyst,
at 2000 K is:
1. 40 × 10−4
2. 4 × 10−4
3. 4 × 10−3
4. Difficult to calculate and need more data
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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Consider the reactions
Correct relationship among the equilibrium constants is:
1. \(\mathrm{K_{3}=K_{1} / K_{2} }\)
2. \(\mathrm{K_{3}=K_{1}^{2} / K_{2}^{2} }\)
3. \(\mathrm{ K_{3}=K_{1} \cdot K_{2}}\)
4. \(\mathrm{K_{3}=K_{1} \cdot \sqrt{K_{2}} }\)
| (i) | \(\mathrm{{CO}(g)+{H}_{2} O(g) \rightleftharpoons {CO}_{2}(g)+{H}_{2}(g) ; K_{1}}\) |
| (ii) | \(\mathrm{CH}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g); K_{2}}\) |
| (iii) | \(\mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{g})+4 \mathrm{H}_{2}(\mathrm{g) ; K_{3}}\) |
1. \(\mathrm{K_{3}=K_{1} / K_{2} }\)
2. \(\mathrm{K_{3}=K_{1}^{2} / K_{2}^{2} }\)
3. \(\mathrm{ K_{3}=K_{1} \cdot K_{2}}\)
4. \(\mathrm{K_{3}=K_{1} \cdot \sqrt{K_{2}} }\)
Subtopic: Introduction To Equilibrium |
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Level 1: 80%+
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