Q. No.\(3A_2+B_2\rightleftharpoons 2A_3B, K_1\\ A_3B \rightleftharpoons \frac 3{2}A_2+\frac 1{2}B_2, K_2 \)
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. | \(K_2=\dfrac 1{\sqrt K_1}\) |
At a given time, the composition of the reaction mixture is : \([\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=2 \times 10^{-3} \mathrm{M} \text {. }\)
In light of the above facts, which of the following is correct?
| 1. | Reaction has a tendency to go in the forward direction. |
| 2. | Reaction has a tendency to go in the backward direction. |
| 3. | Reaction has gone to completion in the forward direction. |
| 4. | Reaction is at an equilibrium. |
(R = 2 cal/mol K)
| 1. | –13.73 cal | 2. | 1372.60 cal |
| 3. | –137.26 cal | 4. | –1381.80 cal |
\(\mathrm{CO_{2}(g)\,+\,C(s)\rightarrow \,2CO(g)}\)
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 |
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 |
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. \(2.4 \times 10^{31} \)
\(\mathrm{N_2(g) +3H_2(g) \rightleftharpoons 2NH_3(g), \Delta H=-Q}\)
Reaction is favoured in forward direction by:
| 1. | Use of catalyst |
| 2. | Decreasing concentration of \(\mathrm{N_2}\) |
| 3. | Low pressure, high temperature and high concentration of ammonia |
| 4. | High pressure, low temperature and higher concentration of \(\mathrm{H_2}\) |
Mark the conditions that favour the maximum product formation in the given reaction.
1. Low temperature and high pressure.
2. Low temperature and low pressure.
3. High temperature and high pressure.
4. High temperature and low pressure.
Consider the reversible exothermic reaction:
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g) + heatUnder which of the following conditions will the equilibrium shift in the forward direction (towards the formation of ammonia)?
1. Increasing the concentration of \(N H_3 ( g )\)2. Decreasing the pressure
3. Decreasing the concentration of \(N_2(g) ~and~H_2(g)\)
4. Increasing the pressure and decreasing the temperature
\(\mathrm{PCl}_5 \leftrightharpoons\mathrm{PCl}_3+\mathrm{Cl}_2\)
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
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