In the equilibrium,

2SO₂(g) + O₂ (g) $\rightleftharpoons$2SO₃(g), the partial pressure of SO₂, O₂ and SO₃ are 0.662, 0.101 and 0.331 atm respectively. What should be the partial pressure of oxygen so that the equilibrium concentration of SO₂ and SO₃ are equal.

1. 0.4 atm                   

2. 1.0 atm

3. 0.8 atm                   

4. 0.25 atm

Ionisation constant of CH₃COOH is 1.7 X 10^-5 and concentration of H⁺ ions is 3.4 X 10^-4.Then, find out initial concentration of CH₃COOH molecules.            

1. 3.4 X 10^-4 

2. 3.4 X 10^-3

3. 6.8 X 10^-4

4. 6.8 X 10^-3

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

The decreasing order of strength of the bases,

OH^-, N${\mathrm{H}}_2^{-}$, H-C$\equiv$C^- and CH₃-C${\mathrm{H}}_2^{-}$ is:

1. CH₃-C${\mathrm{H}}_2^{-}$>N${\mathrm{H}}_2^{-}$> H-C$\equiv$C^->OH^-

2. H-C$\equiv$C^-> CH₃-C${\mathrm{H}}_2^{-}$>N${\mathrm{H}}_2^{-}$>OH^-

3. OH^->N${\mathrm{H}}_2^{-}$>H-C$\equiv$C^->CH₃-C${\mathrm{H}}_2^{-}$

4. N${\mathrm{H}}_2^{-}$>H-C$\equiv$C^->OH^->CH₃-C${\mathrm{H}}_2^{-}$

For the equilibrium, PCl₅ $\rightleftharpoons$ PCl₃ + Cl₂,

${\mathrm{K}}_{\mathrm{C}}={\mathrm{\alpha }}^2/(1-\mathrm{\alpha })\mathrm{V}$, temperature remaining constant:

1. K_c will increase with the increase in volume

2. K_c will increase with the decrease in volume

3. K_c will not change with the change in volume

4. K_c may increase or decrease with the  change in volume depending upon its numerical value.

For the reaction,

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

The forward reaction at constant temperature is favoured by:

1. Introducing an inert gas at a constant volume

2. Introducing chlorine gas at a constant volume

3. Introducing an inert gas at constant pressure

4. None of the above

The reaction quotient (Q) for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right) + 3{\mathrm{H}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by 

$\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ The reaction will proceed towards the right side, if    

1. Q>K_c

2. Q=0

3. Q=K_c

4. Q<K_c

In the dissociation of 2HI $\rightleftharpoons$H₂ + I₂, the degree of dissociation will be influenced by the:

1. Addition of inert gas at constant volume

2. Addition of inert gas at constant pressure

3. Increase of temperature

4. Increase of pressure

Equimolar solutions of the following substances were prepared separetly. Which one of these will record the highest pH value?                                                                                             

1. BaCl₂         

2. AlCl₃         

 3. LiCl           

4. BeCl₂

The correct order of increasing [H₃O⁺] in the following aqueous solutions is:

1. 0.01 M H₂S < 0.01 M H₂SO₄<0.01 M NaCl<0.01M NaNO₂

2. 0.01 M NaCl< 0.01 M NaNO₂<0.01 M H₂S< 0.01 M H₂SO₄

3. 0.01 M NaNO₂<0.01 M NaCl<0.01 M H₂S<0.01 M H₂SO₄

4. 0.01 M H₂S<0.01 M NaNO₂<0.01 M NaCl<0.01 M H₂SO₄