For the reaction $$2 \mathrm{~A} \rightleftharpoons \mathrm{B}+\mathrm{C}, \mathrm{K}_{\mathrm{c}}=4 \times 10^{-3}$$ . At a given time, the composition of reaction mixture is : $$[\mathrm{A}]=[\mathrm{B}]=[\mathrm{G}]=2 \times 10^{-3} \mathrm{M} \text {. }$$
Then, which of the following is correct?
1. Reaction has a tendency to go in forward direction.
2. Reaction has a tendency to go in backward direction.
3. Reaction has gone to completion in forward direction.
4. Reaction is at equilibrium.
Subtopic:  Introduction To Equilibrium |
58%
From NCERT
NEET - 2024
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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:
1. $$K^2_1=2K_2$$
2. $$K_2= \frac { K_1 }{2}$$
3. $$K_1=\frac 1{\sqrt K_2}$$
4. $$K_2=\frac 1{\sqrt K_1}$$
Subtopic:  Introduction To Equilibrium |
72%
From NCERT
NEET - 2024
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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)
 1 –13.73 cal 2 1372.60 cal 3 –137.26 cal 4 –1381.80 cal
Subtopic:  Introduction To Equilibrium |
67%
From NCERT
NEET - 2023
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$$3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g})$$
For the above reaction 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 |
67%
From NCERT
NEET - 2022
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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 |
78%
From NCERT
NEET - 2022
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Kp for the following reaction is 3.0 at 1000 K.
$$\mathrm{CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)}$$
The value of Kfor 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 |
79%
From NCERT
NEET - 2022
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Equilibrium constants K1 and K2 for the following equilibria

are related as:

1.

2. ${\mathrm{K}}_{2}=\frac{{\mathrm{K}}_{1}}{2}$

3.

4. ${\mathrm{K}}_{2}={\mathrm{K}}_{1}^{2}$

Subtopic:  Introduction To Equilibrium |
88%
From NCERT
AIPMT - 2005
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The following equilibria are given:

 $$N_{2} \ + \ 3H_{2} \ \rightleftharpoons \ 2NH_{3}$$ K1 $$N_{2} \ + \ O_{2} \ \rightleftharpoons \ 2NO$$ K2 $$H_{2} \ + \ \frac{1}{2}O_{2} \ \rightleftharpoons \ H_{2}O$$ K3

The equilibrium constant of the reaction
$$2NH_{3} \ + \ \frac{5}{2}O_{2} \ \rightleftharpoons \ 2NO \ + \ 3H_{2}O$$ in terms of K1, K2 and K3 is:

1. K1.K2.K3
2. $$\mathrm{\frac{K_{1}K_{2}}{K_{3}}}$$
3. $$\mathrm{\frac{K_{1}K_{3}^{2}}{K_{3}}}$$
4. $$\mathrm{\frac{K_{2}K_{3}^{3}}{K_{1}}}$$

Subtopic:  Introduction To Equilibrium |
83%
From NCERT
AIPMT - 2003
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