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Q. No.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.
Subtopic: Le Chatelier's principle |
66%
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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 |
80%
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In a gaseous reaction involving \(P, Q \text {, and } R_{,} \text {given } K_c=\frac{[P]^2}{\left[Q[R]^3\right.}\) with \( ΔH<0\), which factor causes
an increase in the equilibrium constant \(K_C\) under constant conditions?
1. An increase in pressure
2. Use of a suitable catalyst
3. A decrease in temperature
4. An increase in temperature
an increase in the equilibrium constant \(K_C\) under constant conditions?
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 |
65%
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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 |
81%
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Consider this ionic equation in an aqueous solution:
CH3O–(aq) + H2O(l) → CH3OH(aq) + OH–(aq)
Which statement about this reaction is correct?
CH3O–(aq) + H2O(l) → CH3OH(aq) + OH–(aq)
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 |
75%
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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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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 |
60%
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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 |
61%
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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 |
67%
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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 |
57%
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