At a given temperature the equilibrium constant for the reaction of:

PCl₅ $\rightleftharpoons$ PCl₃ + Cl₂ is 2.4 × 10^-3. At the same temperature, the equilibrium constant for the reaction

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

• 2.4 × 10^-3

• -2.4 × 10^-3

• 4.2 × 10²

• 4.8 × 10^-2

702.

For the gaseous reaction, C₂H₄ + H₂ $\rightleftharpoons$ C₂H₆; $∆$H = -130 kJ mol^-1 carried in a closed vessel, the equilibrium concentration of the C₂H₆ can definitely be increased by:

• increasing temperature and decreasing pressure

• decreasing temperature and increasing pressure

• increasing temperature and pressure both

• decreasing temperature and pressure both

Which of the following is correct for the reaction?

N₂(g) + 3H₂ (g) $\rightleftharpoons$ 2NH₃ (g)

• K_p = K_c

• K_p < K_c

• K_p > K_c

• Pressure is required to predict the correlation

Among the following, the most acidic is :

• CH₃COOH

• ClCH₂COOH

• Cl₂CHCOOH

• Cl₂CHCH₂COOH

The solubility of CaF₂ in pure water is 2.3 × 10^-4 mol dm³. Its solubility product will be:

• 4.6 × 10^-4

• 4.6 × 10^-8

• 6.9 × 10^-12

• 4.9 × 10^-11

Among BMe₃, BF₃, BCl₃ and B₂H₆ which one will be the best Lewis acid ?

• BCl₃

• BMe₃

• B₂H₆

• BF₃

Which of the following is not a Lewis base ?

• NH₃

• H₂O

• AlCl₃

• None of these

The solubility in water of a sparingly soluble salt AB₂ is 1.0 × 10^-5 mol L^-1. Its solubility product number will be

• 4 × 10^-15

• 4 × 10^-10

• 1 × 10^-15

• 1 × 10^-10

The correct order of increasing basic nature for the bases NH₃, CH₃NH₂ and (CH₃)₂NH is

• CH₃NH₂ < NH₃ < (CH₃)₂NH

• (CH₃)₂NH < NH₃ < CH₃NH₂

• NH₃ < CH₃NH₂ < (CH₃)₂NH

• CH₃NH₂ < (CH₃)₂NH < NH₃

The solubility of CaF₂ in pure water is 2.3 ×10^-6 mol dm^-3. Its solubility product will be:

• 4.8 ×10^-18

• 48.66 ×10^-18

• 4.9 ×10^-11

• 48.66 ×10^-15