Q. No.For the reversible reaction \(A \rightleftharpoons B\), the system is said to be in chemical equilibrium when:
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.
| 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 |
\(\begin{aligned} & \mathrm{NO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \stackrel{\mathrm{K}_1}{\rightleftharpoons} \mathrm{NO}_2(\mathrm{~g}) \text { and } \\ & 2 \mathrm{NO}_2(\mathrm{~g}) \stackrel{\mathrm{K}_2}{\rightleftharpoons} 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \end{aligned}\)
1. \(K_2={1 \over K_1}\)
2. \(K_2={K_1 \over 2}\)
3. \(K_2={1 \over K_1^2}\)
4. \(K_2=K^2_1\)
1. It may be changed by the addition of a catalyst
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
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 |
Given that the equilibrium constant (KC) at 800 K for the reaction \(N_2(𝑔)+3H_2(𝑔)⇋2NH_3(𝑔)\) is 64. What is the equilibrium constant KC at the same temperature for the reaction \(NH_3(g) ⇌ \dfrac{1}{2}N_2(g) + \dfrac{3}{2}H_2(g)\)?
| 1. | \(\dfrac{1}{4}\) | 2. | \(\dfrac{1}{8}\) |
| 3. | 8 | 4. | \(\dfrac{1}{64}\) |
| Assertion (A): | For the reaction, \(Ni(s)+4CO(g)\rightleftharpoons Ni(CO)_4(g)\) the equilibrium constant \(K_c=\frac{[Ni(CO)_4]}{[CO]^4}\) |
| 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. |
For the gaseous equilibrium reaction:
\({N_2O_4 (g) \rightleftharpoons 2NO_2 (g)}\), the equilibrium concentrations of \(\mathrm{N_2O_4}\) and \(\mathrm{NO_2}\) are \(4.8 \times 10^{-2}\) and \(1.2 \times 10^{-2}\), respectively.
Calculate the value of the equilibrium constant \(K_c\) for the reaction:
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
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
| (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) | \(\mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{g})+4 \mathrm{H}_{2}(\mathrm{g) ; K_{3}}\) |
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. \(\mathrm{K_{3}=K_{1} \cdot \sqrt{K_{2}} }\)
© 2026 GoodEd Technologies Pvt. Ltd.