The following equilibria are given

 N₂ + 3H₂ $\rightleftharpoons$ 2NH₃,      K₁

N₂ + O₂ $\rightleftharpoons$ 2NO,          K₂

H₂ + $\frac{1}{2}$O₂ $\rightleftharpoons$ H₂O,       K₃

The equilibrium constant of the reaction, 2NH₃ + $\frac{5}{2}$O₂ $\rightleftharpoons$ 2NO + 3H₂O in terms of  K₁, K₂ and K₃ is  

1. $K_{\mathit{1}}{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_{\mathit{2}}$                       

2. $K_2{K}_{\mathit{3}}^{\mathit{3}}\mathit{/}{K}_1$

3. K₁K₂K₃                            

4. K₁K₂/K₃ 

The pK_a for acid A is greater than pK_a for acid B. The strong acid is:

1. Acid A                                           

2. Acid B

3. Are equally strong                         

4. None of the above

At a certain temperature, 2HI $\rightleftharpoons$H₂ +I₂ only 50% HI is dissociated at equilibrium. The equilibrium constant is:

1. 1.0                     

2. 3.0                 

3. 0.5               

4. 0.25

A solution of FeCl₃ in water acts as acidic due to:

1. Acidic impurities                         

2. Ionization

3. Hydrolysis of Fe³⁺                       

4. Dissociation

Which of the following solution does not act as buffer?

1. H₃PO₄ + NaH₂PO₄

2. Na₂CO₃ + H₂CO₃

3. HCl + NH₄Cl

4. CH₃COOH + CH₃COONa

Which equilibrium can be described as Lewis acid-base reaction but not Bronsted acid-base reaction?

1. H₂O + CH₃COOH$\rightleftharpoons$H₃O⁺ + CH₃COO^-

2. 2NH₃ + H₂SO₄ $\rightleftharpoons$$2{\mathrm{NH}}_4^{+}$ + ${\mathrm{SO}}_4^{2-}$

3. NH₃ + CH₃COOH $\rightleftharpoons$${\mathrm{NH}}_4^{+}$ + CH₃COO^-

4. [Cu(H₂O)₄]²⁺ + 4NH₃ $\rightleftharpoons$ [Cu(NH₃)₄]²⁺ + 4H₂O

In the reaction, PCl₅ $\rightleftharpoons$PCl₃ + Cl₂, the amounts of PCl₅, PCl_3, and Cl₂ at equilibrium are 2 moles each and the total pressure is 3 atm. The equilibrium constant K_p is: 

1. 1.0 atm                                       

2. 2.0 atm

3. 3.0 atm                                       

4. 6.0 atm

An aqueous solution of hydrogen sulphide shows the equilibrium,

           H₂S $\rightleftharpoons$H⁺ + HS^-

If dilute hydrochloric acid is added to an aqueous solution of hydrogen sulphide without any temperature change, then:

When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because:

1. the impurities dissolve in HCl

2. HCl is highly soluble in H₂O

3. the product of [Na⁺] and [Cl^-] exceeds the solubility product of NaCl

4. the solubility product of NaCl is lowered by the chloride ion from aqueous HCl

The aqueous solution of a salt is alkaline. This shows that salt is made from:

1. a strong acid and strong base

2. a strong acid and weak base

3. a weak acid and weak base

4. a weak acid and strong base