Q. No.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
\({N_2O_4 (g) \rightleftharpoons 2NO_2 (g)}\), 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.
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 ionization constant of some weak bases at a particular temperature is given below:
| Base | Dimethylamine | Urea | Pyridine | Ammonia |
| Kb | 5.4 × 10-4 | 1.3 × 10-14 | 1.77 × 10-9 | 1.77 × 10-5 |
The decreasing order of the bases on the extent of their ionization at equilibrium is:
| 1. | Urea > Ammonia > Dimethylamine > Pyridine |
| 2. | Ammonia > Dimethylamine > Pyridine > Urea |
| 3. | Pyridine > Urea > Dimethylamine > Ammonia |
| 4. | Dimethylamine > Ammonia > Pyridine > Urea |
A gaseous compound \({XY_2}\) undergoes dissociation according to the equilibrium:
\(\mathrm{XY}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{XY}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \)
The initial pressure of \({XY_2}\) is 600 mm Hg, and the total pressure at equilibrium is found to be 800 mm Hg. Assuming the volume and temperature of the system remain constant, calculate the value of the equilibrium constant \(K_p\):
1. 502. 100
3. 20
4. 400
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
Find the ratio Kₚ/Kc for the reaction:
CO(g) + ½O₂(g) ⇌ CO₂(g)
1. (RT)1/2
2. (RT)-1/2
3. RT
4. 1
| 1. | RT | 2. | \(\sqrt {RT}\) |
| 3. | \({1 \over RT}\) | 4. | \({ 1 \over \sqrt {RT}}\) |
| 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 |
| Assertion (A): | Addition of \(HCl(aq.)\) to \(HCOOH(aq.)\) decreases the ionization of \(HCOOH(aq.)\) |
| Reason (R): | Due to the common ion effect of \(H^+\), ionization of \(HCOOH \) decreases. |
| 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. | (A) is False but (R) is True. |
| Assertion (A): | The solubility of AgCl in \(NH_3 (aq.) \) is higher than that in pure water. |
| Reason (R): | When AgCl dissolves in \(NH_3 (aq.) \), it forms a complex ion \(\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_2\right]^{+}\), which shifts the solubility equilibrium of AgCl in the forward direction. |
| 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. | (A) is False but (R) is True. |
| Assertion (A): | The solubility of AgCN in acidic solution is greater than that in pure water. |
| Reason (R): | Solubility equilibrium of AgCN in acidic solution is shifted in a forward direction due to the formation of HCN. |
| 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. | (A) is False but (R) is True. |
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