- 1(current)
Q. No.Consider the following reaction in a sealed vessel at equilibrium:
\(2 \text{NO}_{(\text{g})} \rightleftharpoons \text{N}_{2(\text{g})} +\text{O}_{2\text{(g)}}\)
[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
\(2 \text{NO}_{(\text{g})} \rightleftharpoons \text{N}_{2(\text{g})} +\text{O}_{2\text{(g)}}\)
[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
Subtopic: Introduction To Equilibrium |
Level 3: 35%-60%
NEET - 2024
Hints
At a given temperature and pressure, the equilibrium constant value for the equilibria are given below:
\(3A_2+B_2\rightleftharpoons 2A_3B, K_1\\ A_3B \rightleftharpoons \frac 3{2}A_2+\frac 1{2}B_2, K_2 \)
The relation between \(K_1\) and \(K_2\) is:
\(3A_2+B_2\rightleftharpoons 2A_3B, K_1\\ A_3B \rightleftharpoons \frac 3{2}A_2+\frac 1{2}B_2, K_2 \)
The relation between \(K_1\) and \(K_2\) is:
| 1. | \(K^2_1=2K_2\) | 2. | \(K_2= \dfrac { K_1 }{2}\) |
| 3. | \(K_1=\dfrac 1{\sqrt K_2}\) | 4. | \(K_2=\dfrac 1{\sqrt K_1}\) |
Subtopic: Introduction To Equilibrium |
69%
Level 2: 60%+
NEET - 2024
Hints
The equilibrium concentration of the species in the reaction \(A+B \rightleftharpoons C+D\) are 2, 3, 10 and 6 mol L–1, respectively at 300 K. \(\Delta G^o\) for the reaction is:
(R = 2 cal/mol K)
(R = 2 cal/mol K)
| 1. | –13.73 cal | 2. | 1372.60 cal |
| 3. | –137.26 cal | 4. | –1381.80 cal |
Subtopic: Introduction To Equilibrium |
73%
Level 2: 60%+
NEET - 2023
Hints
For the reaction \(3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) \) at 298 K, \(\text K_c\) is found to be \(3.0 \times 10^{-59} \). If the concentration of \(\text O_2\) at equilibrium is 0.040 M, then the concentration of \(\text O_3 \) in M is:
1. \(1.2 \times 10^{21} \)
2. \(4.38 \times 10^{-32} \)
3. \(1.9 \times 10^{-63} \)
4. \(2.4 \times 10^{31} \)
Subtopic: Introduction To Equilibrium |
69%
Level 2: 60%+
NEET - 2022
Hints
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 |
Subtopic: Introduction To Equilibrium | Kp, Kc & Factors Affecting them |
81%
Level 1: 80%+
NEET - 2022
Hints
Kp for the following reaction is 3.0 at 1000 K.
\(\mathrm{CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)}\)
The value of Kc for the reaction at the same temperature is:
(Given: R = 0.083 L bar K–1 mol–1)
\(\mathrm{CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)}\)
The value of Kc for the reaction at the same temperature is:
(Given: R = 0.083 L bar K–1 mol–1)
| 1. | 0.36 | 2. | 3.6 × 10–2 |
| 3. | 3.6 × 10–3 | 4. | 3.6 |
Subtopic: Introduction To Equilibrium |
81%
Level 1: 80%+
NEET - 2022
Hints
- 1(current)
Q. No.
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