Q. No.For the equilibrium reaction:
2NOCl(g) ⇌ 2NO(g) + Cl₂(g)
The equilibrium constant in terms of concentration (Kc) is 3.0 × 10⁻⁶ at 1000 K.
Calculate the value of Kp for the reaction at this temperature.
| 1. | \(1.493\) | 2. | \(2.494\times10^{-2}\) |
| 3. | \(3.0\times10^{-6}\) | 4. | \(2.494\times10^{-4}\) |
\(2 \text{NO}_{(\text{g})} \rightleftharpoons \text{N}_{2(\text{g})} +\text{O}_{2\text{(g)}}\)
[Given: \(\text{N}_2=3.0 \times 10^{-3} \text{M}, \text{O}_2=4.2 \times 10^{-3} \text{M}\) and \(\text{NO}=2.8 \times 10^{-3} \text M\)]
If 0.1 mol L-1 of NO(g) is taken in a closed vessel, what will be the degree of dissociation (\(\alpha\)) of NO(g) at equilibrium?
1. 0.0889
2. 0.00717
3. 0.717
4. 0.00889
At a given time, the composition of the reaction mixture is : \([\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=2 \times 10^{-3} \mathrm{M} \text {. }\)
In light of the above facts, which of the following is correct?
| 1. | Reaction has a tendency to go in the forward direction. |
| 2. | Reaction has a tendency to go in the backward direction. |
| 3. | Reaction has gone to completion in the forward direction. |
| 4. | Reaction is at an equilibrium. |
Match the following equilibria with the corresponding condition.
| 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. | I | II | III | V |
| 3. | V | IV | III | II |
| 4. | IV | V | III | II |
In the reaction, N2O4(g) 2NO2(g), is that part of N2O4 which dissociates. The number of moles at equilibrium will be:
1.
2.
3.
4.
The equilibrium constant Kc expression for the above mentioned reaction is:
| 1. | \(\mathrm{K_{C} = \dfrac{\left[IF_{5}\right]^{2}}{\left[F_{2}\right]^{5}}}\) | 2. | \(\mathrm{K_{C} = \dfrac{\left[IF_{5}\right]^{2}}{\left[F_{2}\right]^{5} \left[I_{2}\right]}}\) |
| 3. | \(\mathrm{K_{C} = \dfrac{\left[F_{2}\right]^{5} \left[I_{2}\right]}{\left[IF_{2}\right]^{2}}}\) | 4. | \(\mathrm{K_{C} = \dfrac{\left[F_{2}\right]^{5}}{\left[IF_{5}\right]^{2}}}\) |
are the respective ionisation constants for the following reactions.
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HS}^{-}\)
\(\mathrm{HS}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{S}^{2-}\)
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{S}^{2-}\)
The correct relationship between is:
1. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} \times \mathrm{K}_{\mathrm{a}_2} \)
2. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1}+\mathrm{K}_{\mathrm{a}_2} \)
3. \(K_{a_3}=K_{a_1}-K_{a_2} \)
4. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} / \mathrm{K}_{\mathrm{a}_2}\)
Reaction quotient for the reaction, is given by , .The reaction will proceed from right to left if Kc value is:
| 1. | Q<Kc | 2. | Q=0 |
| 3. | Q>Kc | 4. | Q=Kc |
| 1. | Equilibrium is possible only in a closed system at a constant temperature. |
| 2. | All measurable properties of the system remain constant. |
| 3. | All the physical processes stop at equilibrium. |
| 4. | The opposing processes occur at the same rate and there is a dynamic but stable condition. |
For a reaction, 2NO (g) + Br2 (g) 2NOBr (g)
When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container of volume 1 litre at a constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The concentration of NO and Br2 at equilibrium will be:
1. NO = 0.0352 mol; = 0.0178 mol
2. NO = 0.352 mol; = 0.178 mol
3. NO = 0.0634 mol; = 0.0596 mol
4. NO = 0.634 mol; = 0.596 mol
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