For a given exothermic reaction K_p and K_p' are the equilibrium constant at temperatures T₁ and T₂ respectively. Assuming that heat of reaction si constant in temperature range between T₁ and T₂ it is readily observed that

• K_p> K_p'

• K_p< K_p'

• K_p = K_p'

• K_p = K_p'

Which of these is least likely to act as a lewis base? 

• CO

• F^-

• BF₃

• BF₃

pH of a saturated solution of Ba(OH)₂ is 12. The value of solubility product K_sp of Ba(OH)₂ is

• 3.3 x 10^-7

• 5.0 x 10^-7

• 4.0 x 10^-6

• 4.0 x 10^-6

Equimolar solutions of the following substances were prepared separately, which one of these will record the highest pH value?

• BaCl₂

• AlCl₃

• LiCl

• LiCl

Buffer solutions have constant acidity and alkalinity because

• these give unionised acid or base on reaction with added acid or alkali

• acids and alkalies in these solutions are shielded from attack by other ions.

• they have a large excess of H⁺ or OH^- ions

• they have a large excess of H⁺ or OH^- ions

Give that the equilibrium constant for the reaction,

2SO₂ (g) + O₂ (g)  ⇌ 2SO₃ (g)

has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction t the same temperature?

SO₃ (g)  ⇌ SO₂ (g) +1/2 O₂ (g)

• 1.8 x 10^-3

• 3.6 x 10^-3

• 6.0 x 10^-2

• 6.0 x 10^-2

Given the reaction between two gases represented by A₂ and B₂ to give the compound AB (g).
A₂(g) +B₂ (g)  ⇌ 2AB (g)
At equilibrium the concentration
of A₂ = 3.0 x 10^-3 M
of B₂ = 4.2 x 10^-3 M
of AB = 2.8 x 10^-3 M

If the reaction takes place in a sealed vessel at 527^oC, then the value of K_c will be

• 2.0

• 1.9

• 0.62

• 0.62

A buffer solution is prepared in which the concentration of NH₃ is 0.30 M and the concentration of NH₄ is 0.20 M. If the equilibrium constant, K_b for NH₃ equals 1.8 x 10^-5, what is the pH of this solution?

log ( 2.7 = 0.43)

• 9.43

• 11.72

• 8.73

• 9.08

789.

The value of ΔH for the reaction

X₂ (g) + 4Y₂ (g) ⇌ 2XY₄ (g) is less than zero. Formation of XY4 (g) will be favoured at

• Low pressure and low temperature

• high temperature and low pressure

• high pressure and low temperature

• high pressure and low temperature

For the reaction N₂ (g) + O₂ (g) ⇌  2NO (g), the equilibrium constant is K₁. The equilibrium constant is K₂ for the reaction 2NO (g) + O₂(g) ⇌ 2NO₂ (g). What is K for the reaction 

• 1/(4K₁K₂)

• [1/K₁K₂]^1/2

• 1/(K₁K₂)

• 1/(K₁K₂)