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Q. No.Given below are two statements:
Assertion (A):
For the reaction, \(Ni(s)+4CO(g)\rightleftharpoons Ni(CO)_4(g)\)
the equilibrium constant \(K_c=\frac{[Ni(CO)_4]}{[CO]^4}\)
Reason (R):
For heterogeneous equilibrium, the concentrations of pure solids or liquids are not considered in the expression of the equilibrium constant.
1.
Both (A) and (R) are True and (R) is the correct explanation of (A).
2.
Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.
(A) is True but (R) is False.
4.
Both (A) and (R) are False.
the equilibrium constant \(K_c=\frac{[Ni(CO)_4]}{[CO]^4}\)
Subtopic: Introduction To Equilibrium |
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For the reversible reaction \(A \rightleftharpoons B\), the system is said to be in chemical equilibrium when:
1. A completely changes to B.2. 50 % of A changes to B.
3. The rate of change of A to B and B to A are the same.
4. Only 10 % of A changes to B.
Subtopic: Introduction To Equilibrium |
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For the reaction:
\(A + B \rightleftharpoons C +D \)If the initial concentrations of A and B are equal. At equilibrium, the concentration of D is found to be twice that of A.
Calculate the value of the equilibrium constant for the reaction:
1. 4/92. 9/4
3. 1/9
4. 4
Subtopic: Introduction To Equilibrium |
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For which of the following reactions \(K_p=K_c \) :
1. \(2 \mathrm{NOCl}(\mathrm{g})=2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{g}) \)
2. \(\mathrm{N}_2(\mathrm{g})+3 \mathrm{H}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{g}) \)
3. \(\mathrm{H}_2(\mathrm{g})+\mathrm{Cl}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{HCl}(\mathrm{g}) \)
4. \(\mathrm{N}_2 \mathrm{O}_4(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{g})\)
1. \(2 \mathrm{NOCl}(\mathrm{g})=2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{g}) \)
2. \(\mathrm{N}_2(\mathrm{g})+3 \mathrm{H}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{g}) \)
3. \(\mathrm{H}_2(\mathrm{g})+\mathrm{Cl}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{HCl}(\mathrm{g}) \)
4. \(\mathrm{N}_2 \mathrm{O}_4(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{g})\)
Subtopic: Kp, Kc & Factors Affecting them |
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Which of the following substances has the strongest acid, given their pH values:
A (9.5), B (2.5), C (3.5), and D (5.5)?
1. A
2. C
3. D
4. B
Subtopic: pH calculation |
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The components of the buffer solution are 0.1 M HCN and 0.2 M NaCN. What is the pH of the solution?
[pKa = 9.3]
1. 9.6
2. 6.15
3. 2.0
4. 4.2
[pKa = 9.3]
1. 9.6
2. 6.15
3. 2.0
4. 4.2
Subtopic: Buffer |
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Identify the correct statement for the equilibrium constant, Keq of a specific reaction:
1. It may be changed by the addition of a catalyst
2. It increases if the concentration of one of the products is increased
3. It changes with changes in the temperature
4. It increases if the concentration of one of the reactants is increased
1. It may be changed by the addition of a catalyst
2. It increases if the concentration of one of the products is increased
3. It changes with changes in the temperature
4. It increases if the concentration of one of the reactants is increased
Subtopic: Introduction To Equilibrium |
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An increase in temperature in an endothermic reversible reaction shifts the equilibrium:
1. Towards the reactant's side
2. Towards the product's side
3. Towards neither of the sides
4. Terminates the reaction
1. Towards the reactant's side
2. Towards the product's side
3. Towards neither of the sides
4. Terminates the reaction
Subtopic: Introduction To Equilibrium |
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An example of homogeneous equilibrium among the following is:
| 1. | \(2SO_{2 (g)} + O_{2(g)} \rightleftharpoons 2SO_3(g)\) |
| 2. | \(C_{(s) }+ H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}\) |
| 3. | \(CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}\) |
| 4. | \(NH_4HS_{(s)} \rightleftharpoons NH_{3(s)} + H_2S_{(g)}\) |
Subtopic: Introduction To Equilibrium |
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Given below are the dissociation constant values of a few acids.
\(H_2SO_3 = 1.3 \times 10^{-2} , HNO_2= 4 \times 10^{-4}, \\ CH_3COOH = 1.8 \times 10^{-5}, HCN = 4 \times 10^{-10}\)
What is the increasing order of acidic strength among the following?
1. \(HCN < CH_3COOH < HNO_2 < H_2SO_3 \)
2. \( CH_3COOH < HNO_2 <HCN< H_2SO_3 \)
3. \( CH_3COOH <HCN< H_2SO_3<HNO_2 \)
4. \(HNO_2 < H_2SO_3 < CH_3COOH < HCN \)
\(H_2SO_3 = 1.3 \times 10^{-2} , HNO_2= 4 \times 10^{-4}, \\ CH_3COOH = 1.8 \times 10^{-5}, HCN = 4 \times 10^{-10}\)
What is the increasing order of acidic strength among the following?
1. \(HCN < CH_3COOH < HNO_2 < H_2SO_3 \)
2. \( CH_3COOH < HNO_2 <HCN< H_2SO_3 \)
3. \( CH_3COOH <HCN< H_2SO_3<HNO_2 \)
4. \(HNO_2 < H_2SO_3 < CH_3COOH < HCN \)
Subtopic: Ionisation Constant of Acid, Base & Salt |
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