What is the relationship between the degree of dissociation (α) of PCl₅ and the pressure at equilibrium in the reaction: PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g)?

1. $\alpha \propto P$                                         

2.  $\alpha \propto 1/\sqrt{P}$

3.  $\alpha \propto 1/{\mathrm{P}}^2$                                   

4.  $\alpha \propto 1/P^4$

The formation of phosgene is represented as,

            CO + Cl₂ $\rightleftharpoons$COCl₂

The reaction is carried out in 500 mL flask. At equilibrium o.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl₂ are present. The equilibrium constant of the reaction is:

1. 30                     

2. 15

3. 5                       

4. 3

If the pressure of N₂ and H₂ mixture in a closed apparatus is 100 atm and 20% of the mixture then reacts, the pressure at  the same temperature would be:

1. 100                   

2. 90

3. 85                     

4. 80

Ostwald's solution dilution law is applicable in the case of the solution of:

1. CH₃COOH                                     

2. NaCl

3. NaOH                                           

4. H₂SO₄

For the reaction, A+B $\rightleftharpoons$3C at 25$°$ C, a 3 litre vessel contains 1, 2, and 4 mole of A, B and C respectively. If K_c for the reaction is 10, then the reaction will proceed in:

1. forward direction                           

2. backward direction

3. in either direction                           

4. in equilibrium

For the reaction, N₂ + 3H₂ $\rightleftharpoons$2NH₃ in a vessel, after the addition of an equal number of mole of N₂ and H₂, the equilibrium state is formed. Which of the following is correct?

1. [H₂] = [N₂]                               

2. [H₂] < [N₂]     

3. [H₂] > [N₂]                                 

4. [H₂] > [NH₃]      

On adding A to the reaction at equilibrium,  AB(s) $\rightleftharpoons$ A(g) + B(g), the new equilibrium concentration of A becomes double, the equilibrium concentration of B would become:

1. 1/2 of its original value

2. 1/4 of it s original value

3. 1/8 of its original value

4. twice of its original value

The relation for calculating pH of a solution containing weak acid and its salt is:

1. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

2. pH = pK_a - log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

3. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Salt}\right]}$

4. pOH = pK_a - log$\frac{\left[\mathrm{Acid}\right]}{[\mathrm{Conjugate} \mathrm{Base}]}$

The equilibrium constants for the reaction,

A₂ $\rightleftharpoons$2A at 500 K and 700 K are 1x10^-10 and 1x10^-5. The given reaction is                  

(a) exothermic                    (b) slow

(c) endothermic                  (d) fast

1. a,b

2.c,b

3.a,d

4 c,d

A solution is called saturated if:

1. ionic concentration product < solubility product

2. ionic concentration product > solubility product

3. ionic concentration product $\ge$ solubility product

4. none of the above