Q. No.For a given reaction, \( K_P=9~\text{atm}\)
\(\mathrm{NH}_{3(\mathrm{~g})} \rightleftharpoons \frac{1}{2} \mathrm{~N}_{2(\mathrm{~g})}+\frac{3}{2} \mathrm{H}_{2(\mathrm{~g})}\)
Total pressure at equilibrium is \(\sqrt 3\) atm.
Find the value of \(7~\alpha ^2,\) where \(\alpha \) is degree of dissociation of \(NH_{3(g)}?\)
1. 2.8
2. 5.2
3. 5.6
4. 8.4
\(\mathrm{NH}_{3(\mathrm{~g})} \rightleftharpoons \frac{1}{2} \mathrm{~N}_{2(\mathrm{~g})}+\frac{3}{2} \mathrm{H}_{2(\mathrm{~g})}\)
Total pressure at equilibrium is \(\sqrt 3\) atm.
Find the value of \(7~\alpha ^2,\) where \(\alpha \) is degree of dissociation of \(NH_{3(g)}?\)
1. 2.8
2. 5.2
3. 5.6
4. 8.4
Subtopic: Kp, Kc & Factors Affecting them | Ionisation Constant of Acid, Base & Salt |
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For a given reaction at 400 K:
(R=0.082 atm-L/mol-K)
\(\mathrm{xA} \rightleftharpoons \mathrm{yB}\)
Given:
(i) \( \mathrm{K}_{\mathrm{p}}=0.82, \mathrm{~K}_{\mathrm{c}}=25.7\)
(ii) \(\mathrm{K}_{\mathrm{P}}=8.2, \mathrm{~K}_{\mathrm{c}}=0.25\)
Then what is the correct combination of x & y for above set (i) & set (ii) data:
(R=0.082 atm-L/mol-K)
\(\mathrm{xA} \rightleftharpoons \mathrm{yB}\)
Given:
(i) \( \mathrm{K}_{\mathrm{p}}=0.82, \mathrm{~K}_{\mathrm{c}}=25.7\)
(ii) \(\mathrm{K}_{\mathrm{P}}=8.2, \mathrm{~K}_{\mathrm{c}}=0.25\)
Then what is the correct combination of x & y for above set (i) & set (ii) data:
| set (i) (x,y) |
set (ii) (x,y) |
|
| 1. | (1,2) | (2,1) |
| 2. | (2,1) | (1,2) |
| 3. | (1,1) | (2,1) |
| 4. | (1,2) | (1,1) |
Subtopic: Kp, Kc & Factors Affecting them |
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At temperature T, compound \(\mathrm{AB}_{2(\mathrm{~g})}\) dissociates as \(\mathrm{AB}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{AB}_{(\mathrm{g})}+\frac{1}{2} \mathrm{~B}_{2(\mathrm{~g})} \) , having degree of dissociation x (small compared to unity). The correct expression for x in terms of Kp and p is:
| 1. | \(\sqrt[3]{\frac{2 K_p}{p}} \) | 2. | \(\sqrt[4]{\frac{2 \mathrm{~K}_{\mathrm{p}}}{\mathrm{p}}}\) |
| 3. | \(\sqrt[3]{\frac{2 \mathrm{~K}_{\mathrm{p}}^2}{\mathrm{p}}} \) | 4. | \(\sqrt{\mathrm{K}_{\mathrm{p}}} \) |
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the reaction:
\(\mathrm{X}_2 \mathrm{Y}(\mathrm{~g}) \rightleftharpoons \mathrm{X}_2(\mathrm{~g})+\frac{1}{2} \mathrm{Y}_2(\mathrm{~g})\)
The equation representing the correct relationship between the degree of dissociation (x) of X2Y(g) with its equilibrium constant Kp is:
(Assume x to be very very small)
\(\mathrm{X}_2 \mathrm{Y}(\mathrm{~g}) \rightleftharpoons \mathrm{X}_2(\mathrm{~g})+\frac{1}{2} \mathrm{Y}_2(\mathrm{~g})\)
The equation representing the correct relationship between the degree of dissociation (x) of X2Y(g) with its equilibrium constant Kp is:
(Assume x to be very very small)
| 1. | \(\mathrm{x}=\sqrt[3]{\dfrac{2 \mathrm{Kp}}{\mathrm{p}}}\) | 2. | \(x=\sqrt[3]{\dfrac{2 \mathrm{Kp}^2}{\mathrm{p}}}\) |
| 3. | \(x=\sqrt[3]{\dfrac{\mathrm{Kp}}{2 \mathrm{p}}}\) | 4. | \(x=\sqrt[3]{\dfrac{K p}{p}}\) |
Subtopic: Kp, Kc & Factors Affecting them | Ionisation Constant of Acid, Base & Salt |
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Calculate the equilibrium constant Kp for the reaction
\(2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_{4(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)
at 500 K, given that 37.8 g of N2O5 was placed in a 1 L reaction vessel, and the total pressure at equilibrium was found to be 18.65 bar.
[Assume N2O5 to behave ideally under these conditions]
[Given : R = 0.082 bar L mol–1 K–1 ]
1. 96.2
2. 6.75
3. 9.619
4. 18.6
\(2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_{4(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)
at 500 K, given that 37.8 g of N2O5 was placed in a 1 L reaction vessel, and the total pressure at equilibrium was found to be 18.65 bar.
[Assume N2O5 to behave ideally under these conditions]
[Given : R = 0.082 bar L mol–1 K–1 ]
1. 96.2
2. 6.75
3. 9.619
4. 18.6
Subtopic: Kp, Kc & Factors Affecting them |
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Find relation between \(\mathrm{K_P}\) and \(\mathrm{K_C}\) for this given reaction:
\(\mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}(\mathrm{g})\)
1. \(K_P=K_C(R T)^1 \)
2. \( K_P=K_C(R T)^{-1}\)
3. \(K_P=K_C(R T)^{1 / 2} \)
4. \( K_P=K_C(R T)^{-1 / 2}\)
\(\mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}(\mathrm{g})\)
1. \(K_P=K_C(R T)^1 \)
2. \( K_P=K_C(R T)^{-1}\)
3. \(K_P=K_C(R T)^{1 / 2} \)
4. \( K_P=K_C(R T)^{-1 / 2}\)
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the following equilibrium reaction:
\(\mathrm{H}_2+\mathrm{I}_2 \rightleftharpoons 2 \mathrm{HI}\)
At equilibrium, if the number of molecules of \(\mathrm{H}_2,~ \mathrm{I}_2,\) and \(\mathrm{HI}\) are equal, and the equilibrium constant \(\mathrm{K}_{\mathrm{p}}=\mathrm{t} \times 10^{-1}\), the value of t is:
\(\mathrm{H}_2+\mathrm{I}_2 \rightleftharpoons 2 \mathrm{HI}\)
At equilibrium, if the number of molecules of \(\mathrm{H}_2,~ \mathrm{I}_2,\) and \(\mathrm{HI}\) are equal, and the equilibrium constant \(\mathrm{K}_{\mathrm{p}}=\mathrm{t} \times 10^{-1}\), the value of t is:
| 1. | 10.0 | 2. | 0.01 |
| 3. | 0.10 | 4. | 1.0 |
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the following reaction at equilibrium at a temperature of T Kelvin, with a given equilibrium constant \(K_c=3 \times 10^{-13}:\)
\(\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})\)
Now, consider the reverse reaction:
\(2 \mathrm{SO}_3(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\)
The equilibrium constant for this reaction is denoted as \(K_{c^{\prime}}^{\prime}\) which can be expressed as \(a \times 10^{+b}\) in scientific notation.
What is the value of \(a+b\) ?
1. 26
2. 29
3. 20
4. 19
\(\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})\)
Now, consider the reverse reaction:
\(2 \mathrm{SO}_3(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\)
The equilibrium constant for this reaction is denoted as \(K_{c^{\prime}}^{\prime}\) which can be expressed as \(a \times 10^{+b}\) in scientific notation.
What is the value of \(a+b\) ?
1. 26
2. 29
3. 20
4. 19
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the following equilibrium reactions along with their respective equilibrium constants:
\(\begin{aligned} & x \rightleftharpoons y~ ;~~ k_1=1 \\ & y \rightleftharpoons z ~; ~~k_2=2 \\ & z \rightleftharpoons w~ ; ~~k_3=4 \end{aligned}\)
Now, calculate the overall equilibrium constant \(k_{\text{eq}}\) for the reaction:
\( \mathrm{x} \rightleftharpoons \mathrm{w}\)
Choose the correct answer:
\(\begin{aligned} & x \rightleftharpoons y~ ;~~ k_1=1 \\ & y \rightleftharpoons z ~; ~~k_2=2 \\ & z \rightleftharpoons w~ ; ~~k_3=4 \end{aligned}\)
Now, calculate the overall equilibrium constant \(k_{\text{eq}}\) for the reaction:
\( \mathrm{x} \rightleftharpoons \mathrm{w}\)
Choose the correct answer:
| 1. | 10 | 2. | 8 |
| 3. | 2 | 4. | 4 |
Subtopic: Kp, Kc & Factors Affecting them |
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\(\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})+\dfrac{1}{2} \mathrm{C}(\mathrm{g}) \)
In the above reaction, the correct relation among \( \text{K}_p\), \( \alpha\) and equilibrium pressure (p) is:
1. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{1 / 2} 2 \mathrm{p}^{1 / 2}}{(2+\alpha)^{1 / 2}}\)
2. \(K_p=\dfrac{\alpha^{1 / 2} p^{3 / 2}}{(2+\alpha)^{3 / 2}}\)
3. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{1 / 2} 2 \mathrm{p}^{1 / 2}}{(2+\alpha)^{3 / 2}}\)
4. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{3 / 2} \mathrm{p}^{1 / 2}}{(2+\alpha)^{1 / 2}(1-\alpha)}\)
Subtopic: Kp, Kc & Factors Affecting them |
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