Match the following equilibria with the corresponding condition.
A. | LiquidVapour | 1. | Saturated solution |
B. | SolidLiquid | 2. | Boiling point |
C. | SolidVapour | 3. | Sublimation point |
D. | Solute (s)Solute (solution) | 4. | Melting point |
5. | Unsaturated solution |
Codes:
A | B | C | D | |
1. | 2 | 4 | 3 | 1 |
2. | 1 | 2 | 3 | 5 |
3. | 5 | 4 | 3 | 2 |
4. | 4 | 5 | 3 | 2 |
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. \(\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} / \mathrm{K}_{\mathrm{a}_2}\)
If the molar concentration of is mol L–1, the concentration of chloride ions will be:
1. | 3.0 x 10-3 | 2. | 6.0 x 10-3 |
3. | 0.3 x 10-3 | 4. | 0.6 x 10-6 |
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 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
In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:
1. | 4 | 2. | 16 |
3. | 2 | 4. | 1 |
Which of the following is an example of a reversible reaction?
1. | \(\small{KNO_3(aq) + NaCl(aq) \rightleftharpoons KCl(aq) + NaNO_3(aq)} \) |
2. | \(\small{2Na(s) + H_2O(l) \rightleftharpoons 2NaOH(aq) + H_2(g)} \) |
3. | \(\small{AgNO_3(aq) + NaCl(aq) \rightleftharpoons AgCl(s) + NaNO_3(aq)} \) |
4. | \(\small{Pb{(NO_3)}_2(aq) + 2NaI(aq) \rightleftharpoons PbI_2(s) + 2NaNO_3(aq)} \) |