# 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 |
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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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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

 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
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
Subtopic:  Ionisation Constant of Acid, Base & Salt |
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To view explanation, please take trial in the course.
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To view explanation, please take trial in the course.
NEET 2025 - Target Batch

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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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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