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

40% of a racemic mixture of 0.2 moles of N₂ and 0.6 moles of H₂ react to give NH₃ according to the equation, N₂ (g) + H₂(g)$\rightleftharpoons$2NH₃ (g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is:

1. 4:5                       

2. 5:4

3. 7:10                     

4. 8:5

On addition of inert gas at constant volume to the reaction, N₂ + 3H₂$\rightleftharpoons$2NH₃ at  equilibrium:

1. the reaction halts

2. forward reaction is favored

3. the reaction remains unaffected

4. backward reaction is favored

In which of the following case reaction goes farthest to completion?

1. K=10³                                         

2. K=10^-2

3. K=10                                           

4. K=10⁰

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