Q. No.PCl5, PCl3, and Cl2 are at equilibrium at 500 K in a closed container and their concentrations are 0.8×10–3 mol L–1 , 1.2×10–3 mol L–1 and 1.2×10–3 mol L–1, respectively.
The value of Kc for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) will be:
1. 1.8 × 103 mol L–1
2. 1.8 × 103
3. 1.8 × 10–3 mol L–1
4. 0.55 × 104
Find the equilibrium constant (Kc) at 500 K for:
2HI(g) ⇌ H₂(g) + I₂(g)
given that:
½H₂(g) + ½I₂(g) ⇌ HI(g), Kc = 5
1. 0.04
2. 0.4
3. 25
4. 2.5
Find the equilibrium constant Kc for the reaction:
H₂O(g) + CO(g) ⇌ H₂(g) + CO₂(g)
Initially, 1 mol each of H₂O and CO are taken in a 10 L vessel at 725 K. At equilibrium, 40% of H₂O reacts.
| 1. | 0.66 | 2. | 0.35 |
| 3. | 0.44 | 4. | 0.82 |
A sample of pure PCl5 was introduced into an evacuated vessel at 473 K.
After equilibrium was attained, a concentration of PCl5
was found to be 0.5 × 10–1 mol L–1. If the value of
Kc is 8.3 × 10–3 mol L–1, the concentrations of
PCl3 and Cl2 at equilibrium would be:
PCl5 (g) PCl3 (g) + Cl2(g)
| 1. | |
| 2. | |
| 3. | |
| 4. |
Match the following reactions with the corresponding equilibrium constant:
| Column-I (Reaction) | Column-II (Equilibrium constant) | ||
| A. | (i) | ||
| B. | (ii) | ||
| C. | (iii) | ||
| (iv) |
(Given that reference, Kc is the equilibrium constant for the ammonia synthesis.)
Codes:
| A | B | C | |
| 1. | (iv) | (iii) | (ii) |
| 2. | (i) | (ii) | (iii) |
| 3. | (i) | (iv) | (iii) |
| 4. | (iv) | (i) | (iii) |
Consider the following reaction taking place in 1L capacity container at 300 K.
\(\mathrm{A +B \rightleftharpoons C+D }\)
If one mole each of A and B are present initially and at equilibrium 0.7 mol of C is formed, then the equilibrium constant \((K_c) \) for the reaction is:
| 1. | 9.7 | 2. | 1.2 |
| 3. | 6.2 | 4. | 5.4 |
\(\mathrm{PCl}_5 \leftrightharpoons\mathrm{PCl}_3+\mathrm{Cl}_2\)
At equilibrium at \(500 \mathrm{~K},\) the concentration of \(\mathrm{PCl}_5=1.40~ \mathrm{M} \text {, }\) concentration of \(\mathrm{Cl}_2=1.60~ \mathrm{M} \text {, }\) concentration of \(\mathrm{PCl}_3=1.60 \mathrm{M}\). Calculate \(K_c\):
1. 2.00
2. 2.6
3. 1.83
4. 3.4
Given the reaction 2HI (g) H2 (g) + I2 (g)
A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, the partial pressure of HI(g) is 0.04 atm. The for the given equilibrium would be:
| 1. | 2.0 | 2. | 3.5 |
| 3. | 4.0 | 4. | 2.6 |
| 1. | \(\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{(\mathrm{g})}\) |
| 2. | \(\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}\) |
| 3. | \(2 \mathrm{BrCl}_{(\mathrm{g})} \rightleftharpoons \mathrm{Br}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}\) |
| 4. | \(\mathrm{PCl}_{5(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}\) |
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. | \(2.494\times10^{-4}\) |
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