For the reversible reaction,

N₂ (g) + 3H₂(g) $\rightleftharpoons$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

 

The correct representation for the solubility product constant of Ag₂CrO₄ is:

1. [Ag⁺]²[${\mathrm{CrO}}_4^{2-}$]                             

2. [Ag²⁺][${\mathrm{CrO}}_4^{2-}$]

3. [2Ag⁺][${\mathrm{CrO}}_4^{2-}$]                             

4. [2Ag⁺]²[${\mathrm{CrO}}_4^{2-}$]

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product K_sp 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

At a given temperature the K_c for the reaction,

PCl₅ (g) $\rightleftharpoons$ PCl₃ (g) + Cl₂ (g) is 2.4 x10^-3. At the same temperature, the K_c for the reaction

PCl₃ (g) + Cl₂ (g) $\rightleftharpoons$ PCl₅ (g)  is :

1. 2.4x10^-3           

2. -2.4 x10^-3

3. 4.2 x10²           

4.  4.8 x10^-2

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 :

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

The strongest acid among the following is:          

1. H₂SO₄           

_2. HClO₃       

3. HClO₄         

4. H₂SO₃ 

pH for the solution of salt undergoing anionic hydrolysis (say CH₃COONa) is given by:

1. pH = $\frac{1}{2}$[pK_w + pK_a + log c]

2. pH = $\frac{1}{2}$[pK_w + pK_a - log c]

3. pH = $\frac{1}{2}$[pK_w + pK_b - log c]

4. none of the above

Which can act as an acidic buffer?

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

The following equilibrium exists in an aqueous solution 

CH₃COOH $\rightleftharpoons$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