If the equilibrium constant for N₂(g)+O₂(g)$\rightleftharpoons$2NO(g) is K, the equilibrium constant for

$\frac{1}{2}$N₂(g) + $\frac{1}{2}$O₂(g)$\rightleftharpoons$NO(g) will be,

1. K^1/2

2. $\frac{1}{2}K$

3. K

4. K²

For the reversible reaction, N₂(g) + 3H₂(g) — 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 decreasing temperature

For a given exothermic reaction, K_p and K'_p are the equilibrium constants at temperatures

T₁ and T₂ respectively. Assuming that heat of reaction is constant in a temperature range

between T₁ and T₂, it is readily observed that

1. K_p>K'_p                       

2. K_p<K'_p

3. K_p = K'_p                     

4. K_p = 1/K'_p

Buffer solutions have constant acidity and alkalinity because
1. these give unionised acid or base or base on reaction with added acid or alkali
2. acids and alkalies in these solutions are shielded from attack by other ions
3. they have large excess of H⁺ or OH^- ions
4. they have fixed value of pH

The molecule that is least likely to behave as Lewis base is: 

1. NH₃

2. BF₃

3. OH^-

4. H₂O

K_c and K_p are not equal for a reaction given below:

1. 2NO(g) $\rightleftharpoons$N₂(g) + O₂(g)

2. SO₂(g) + NO₂(g) $\rightleftharpoons$SO₃(g) + NO(g)

3. H₂(g) + I₂(g) $\rightleftharpoons$2HI(g)

4. 2C(s) + O₂(g) $\rightleftharpoons$2CO₂(g)

Which one of the following molecular hydrides acts as a Lewis acid?

1. NH₃         

2. H₂O         

3. B₂H₆           

4. CH₄

Which of the following molecules acts as a Lewis acid ?

1. (CH₃)₃B

2. (CH₃)₂O

3. (CH₃)₃P

4. (CH₃)₃N

The ionisation constant of ammonium hydroxide is 1.77 x 10^-5 at 298 K. Hydrolysis constant of ammonium chloride is

1. 5.65 x 10^-10

2. 6.50 x 10^-12

3. 5.65 x 10^-13

4. 5.65 x 10^-12

The oxide that is not expected to react with sodium hydroxide is : 

1. B₂O₃           

2. CaO

3. SiO₂             

4. BeO