Q. No.\(K_p\) for the reaction at \(1000~ K\) is:
[ Given: \({R= 0.0831~ L ~\text{atm mol}^{-1} }K^{-1}]\)
1. \(0.033 \)
2. \(0.021 \)
3. \(83.1 \)
4. \(2 .077 \times 10^5\)
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. |
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. \(\mathrm{PCl}_{5(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}\)
\(\mathrm{PCl}_5=\mathrm{PCl}_3+\mathrm{Cl}_2\)
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
\(\mathrm{2NOCl_\text{(g)}\rightleftharpoons2NO_{\text{(g)}}+Cl_{2{\text{(g)}}}}\)
the value of the equilibrium constant is \(3.0\times10^{-6} \) at \(1000~K.\) Find \(K_p\) for the reaction at this temperature (Given \(R:8.314~\text{J K}^{-1}\text{mol}^{-1}\)):
| 1. | \(1.493\) | 2. | \(2.494\times10^{-2}\) |
| 3. | \(3.0\times10^{-6}\) | 4. | \(2.494\times10^{-4}\) |
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 |
Based on the given equilibrium constants:
\( \begin{array}{lc} \mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3 & \mathrm{~K}_1 \\ \mathrm{~N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO} & \mathrm{K}_2 \\ \mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O} & \mathrm{K}_3 \end{array} \)
The equilibrium constant (K) of the following reaction will be:
\(2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \stackrel{\mathrm{~K}}{\rightleftharpoons} 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O}\)
| 1. | \( \dfrac{K_{2}K_{3}^{3}}{K_{1}}\) | 2. | \( \dfrac{K_{2}K_{3}}{K_{1}}\) |
| 3. | \( \dfrac{K_{2}^{3}K_{3}}{K_{1}}\) | 4. | \( \dfrac{K_{3}^{3}K_{1}}{K_{2}}\) |
A 20-litre container at 400 K contains CO2 (g) at pressure 0.4 atm and an excess of SrO (neglecting the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container.
The maximum volume of the container, when the pressure of CO2 attains its maximum value will be:
(Given that: SrCO3(s) ⇋ SrO(s) + CO2(g) , Kp = 1.6 atm)
| 1. | 10 litre | 2. | 2 litre |
| 3. | 4 litre | 4. | 5 litre |
If the equilibrium constant for N2(g) + O2 (g) ⇄ 2NO(g) is K, the equilibrium constant for \(\frac{1}{2}\)N2(g) + \(\frac{1}{2}\)O2(g) ⇄ NO(g) will be?
1.
2.
3. K
4.
The value of the equilibrium constant for a particular reaction is 1.6 × 1012. When the system is in equilibrium, it will include:
1. All reactants
2. Mostly reactants
3. Mostly products
4. Similar amounts of reactants and products
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