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 equilibrium constants for the reactions are:

H₃PO₄ $\stackrel{K_{\mathit{1}}}{\rightleftharpoons }$H+ + H₂P${\mathrm{O}}_4^{-}$;                      K₁

H₂P${\mathrm{O}}_4^{-}$$\stackrel{K_{\mathit{2}}}{\rightleftharpoons }$H+ + HP${\mathrm{O}}_4^{2-}$;                      K₂

HP${\mathrm{O}}_4^{2-}$$\stackrel{K_{\mathit{3}}}{\rightleftharpoons }$H+ + P${\mathrm{O}}_4^{3-}$                        K₃

The equilibrium constants for 

H₃PO₄$\rightleftharpoons$3H+ + P${\mathrm{O}}_4^{3-}$  will be:

1. K₁/K₂K₃                                         

2. K₁xK₂xK₃

3. K₂/K₁K₃                                       

4. K₁+K₂+K₃

The equilibrium constant for the reaction,

SO₃ (g) $\rightleftharpoons$SO₂(g) + $\frac{1}{2}$O₂(g); K_c = 4.9 x 10^-2.

The K_c for the reaction: 2SO₂(g) + O₂(g) $\rightleftharpoons$2SO₃(g) will be:

1. 416.5                             

2. 2.40 x10^-3

3. 9.8 x10^-2                       

4. 4.9 x10^-2

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