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Q. No.P, Q, and R represent substances involved in a gaseous reaction.
The equilibrium constant (Kc ) and the sign of the enthalpy change for the reaction are:
\(K_c = \frac{[P]^2}{[Q][R]3}~~~~~~\Delta H ~ is ~negative \)
Assuming that all other conditions remain constant, a change in which factor results in an increase of the value of the equilibrium constant, Kc?
1. an increase in pressure
2. use of a suitable catalyst
3. a decrease in temperature
4. an increase in temperature
Subtopic: Introduction To Equilibrium |
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X and Y are acidic solutions. X has a pH of 2 and Y has a pH of 4. Which of the following statements about hydrogen ion concentrations of X and Y is correct?
| 1. | Y has a hydrogen ion concentration 2 times greater than X. |
| 2. | X has a hydrogen ion concentration 100 times greater than Y. |
| 3. | X has a hydrogen ion concentration 4 times greater than Y |
| 4. | Y has a hydrogen ion concentration 100 times greater than X |
Subtopic: pH calculation |
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Consider this ionic equation in an aqueous solution:
CH3O– + H2O → CH3OH + OH–
Which statement about this reaction is correct?
CH3O– + H2O → CH3OH + OH–
Which statement about this reaction is correct?
| 1. | CH3OH is the conjugate acid of CH3O-. |
| 2. | The CH3O– ion is a Lewis acid. |
| 3. | The final mixture of solutions would have a pH below 7. |
| 4. | Water is acting as a Bronsted–Lowry base. |
Subtopic: Acids & Bases - Definitions & Classification |
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If the solubility product of Pb3(PO4)2 is 1.5 × 10-32, then the solubility in gm/litre is-
(Given: Molecular mass of Pb3(PO4)2 = 811 g/mol)
1. 2.92 × 10-7
2. 4.94 × 10-12
3. 7.42 × 1034
4. 1.37 × 10-4
(Given: Molecular mass of Pb3(PO4)2 = 811 g/mol)
1. 2.92 × 10-7
2. 4.94 × 10-12
3. 7.42 × 1034
4. 1.37 × 10-4
Subtopic: Solubility Product |
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Identify that is NOT an example of heterogeneous equilibrium:
| 1. | Equilibrium between water vapour and liquid water in a closed container |
| 2. | Equilibrium attained during acid catalysed hydrolysis of ethyl acetate |
| 3. | Equilibrium between solid Ca(OH)2 and its saturated solution |
| 4. | Equilibrium attained on heating solid CaCO3 in a closed container |
Subtopic: Introduction To Equilibrium |
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| Assertion (A): | Sparingly soluble salts AB and XY2 with the same solubility product, will have different solubility. |
| Reason (R): | Solubility of sparingly soluble salt depend upon solubility product as well as the type of salt. |
| 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. | (A) is false but (R) is true. |
Subtopic: Solubility Product |
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On adding inert gas at constant volume, equilibrium shifts in the forward direction will take place in -
1. \(N_2 (g) + 3H_2 (g)\rightleftharpoons 2NH_3 (g)\)
2. \(PCl_5 (g) \rightleftharpoons PCl_3 (g) + Cl_2 (g)\)
3. \(H_2(g) + I_2 (g) \rightleftharpoons 2HI (g)\)
4. None of the above.
1. \(N_2 (g) + 3H_2 (g)\rightleftharpoons 2NH_3 (g)\)
2. \(PCl_5 (g) \rightleftharpoons PCl_3 (g) + Cl_2 (g)\)
3. \(H_2(g) + I_2 (g) \rightleftharpoons 2HI (g)\)
4. None of the above.
Subtopic: Le Chatelier's principle |
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The ionization constant of ammonia is 1.77 × 10–5. The pH of a 0.05M of ammonia solution is 11. The ionization constant of the conjugate acid of ammonia is:
1. 2.44 × 10–9
2. 6.14 × 10–12
3. 1.24 × 10–14
4. 5.64 × 10–10
1. 2.44 × 10–9
2. 6.14 × 10–12
3. 1.24 × 10–14
4. 5.64 × 10–10
Subtopic: Ionisation Constant of Acid, Base & Salt |
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At 4oC , ionic product of water (K\(\omega\)) is 10-16 . At this temperature, a solution has pH = 7.5 . The nature of this solution at 4oC will be
1. Acidic
2. Alkaline
3. Neutral
4. Cannot be predicted
Subtopic: pH calculation |
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For the given reaction: H2NCOONH4 (s) \( \rightleftharpoons\) 2NH3 (g) + CO2 (g),
total pressure at equilibrium is found to be 18 atmospheres. The value of Kp for the above equilibrium will be
1. 72 atm3
2. 144 atm3
3. 432 atm3
4. 864 atm3
Subtopic: Introduction To Equilibrium |
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