For the reversible reaction,

N2 (g) + 3H2(g) 2NH3 (g) + heat

 the equilibrium shifts in forward direction                                   

1. by increasing the concentration of NH3 (g) 

2. by decreasing the pressure

3. by decreasing the concentrations of N2 (g)and H2(g)

4. by increasing pressure and decreassing temperature

 

Subtopic:  Le Chatelier's principle |
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The correct representation for the solubility product constant of Ag2CrO4 is:

1. [Ag+]2[CrO42-]                             

2. [Ag2+][CrO42-]

3. [2Ag+][CrO42-]                             

4. [2Ag+]2[CrO42-]

Subtopic:  Solubility Product |
 51%
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pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product Ksp of Ba(OH)2 is

1. 3.3 x 10-7                         

2. 5.0 x 10-7

3. 4.0 x 10-6                         

4.  5.0 x 10-6

Subtopic:  Solubility Product |
 60%
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At a given temperature the Kc for the reaction,

PCl5 (g PCl3 (g) + Cl2 (g) is 2.4 x10-3. At the same temperature, the Kc for the reaction

PCl3 (g) + Cl2 (g PCl5 (g)  is :

1. 2.4x10-3           

2. -2.4 x10-3

3. 4.2 x10          

4.  4.8 x10-2

Subtopic:  Kp, Kc & Factors Affecting them |
 78%
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HI was heated in a sealed tube at 440°C till the equilibrium was reached. At this point, HI was found to be 22 % decomposed. The equilibrium constant for this dissociation is :

1. 0.28 2. 0.08
3. 0.02 4. 1.99
Subtopic:  Introduction To Equilibrium |
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28 g N2 and 6g H2 were mixed. At equilibrium 17 g NH3 was formed. the mass of N2 and H2 of equilibrium are respectively:

1. 11 g, zero                             

2. 1 g, 3 g

3. 14 g, 3 g                                 

4. 11 g, 3 g

Subtopic:  Introduction To Equilibrium |
 75%
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The strongest acid among the following is:          

1. H2SO4           

2. HClO3       

3. HClO4         

4. H2SO3 

Subtopic:  Acids & Bases - Definitions & Classification |
 70%
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pH for the solution of salt undergoing anionic hydrolysis (say CH3COONa) is given by:

1. pH = 12[pKw + pKa + log c]

2. pH = 12[pKw + pKa - log c]

3. pH = 12[pKw + pKb - log c]

4. none of the above

Subtopic:  Salt Hydrolysis & Titration |
 64%
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Which can act as an acidic buffer?

a. NH4Cl + NH4OH
b. CH3COOH + CH3COONa
c. 40 mL of 0.1 M NaCN + 20 mL of 0.1 M HCl


1. Both a and b
2. Both b, and c
3. All are buffer solution
4. Both a, and c

Subtopic:  Buffer |
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The following equilibrium exists in an aqueous solution 

CH3COOH H+ + CH3COO- . If dilute HCl is added to this solution:

1. the equilibrium constant will increase

2. the equilibrium constant will decrease

3. acetate ion concentration will increase

4. acetate ion concentration will decrease

Subtopic:  Ionisation Constant of Acid, Base & Salt |
 71%
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