For a spontaneous reaction the ∆G, equilibrium constant (K) and E^o_cell will be respectively 

• -ve, >1, +ve

• +ve, >1, -ve

• -ve, <1, -ve

• -ve, <1, -ve

The exothermic formation of ClF₃ is represented by the equation


Which of the following will increase the quantity of ClF₃ in an equilibrium mixture of Cl₂, F₂ and ClF₃?

• Increasing the temperature

• Removing Cl₂

• Increasing the volume of the container

• Increasing the volume of the container

For the reaction



When K_p and K_c are compared at 184^oC, it is found that

• K_p is greater than K_c

• K_p is less than K_c

• K_p = K_c

• K_p = K_c

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be

• 3.98 x 10⁸

• 3.88 x 10⁶

• 3.68 x 10^-6

• 3.68 x 10^-6

What is the conjugate base of OH^-?

• O₂

• H₂O

• O^-

• O^-

Among the following acids which has the lowest p_Ka value?

• CH₃COOH

• HCOOH

• (CH₃)₂COOH

• (CH₃)₂COOH

The conjugate base of H₂PO₄^- is

• PO₄^3-

• HPO₄^2-

• H₃PO₄

• H₃PO₄

What is the equilibrium expression for the reaction P₄(s) +5O₂(g)⇌ P₄O₁₀(s)? 

• Kc = [P₄O₁₀] / P₄] [O₂]⁵

• K_c = 1/[O2]⁵

• K_c = [O2] 5

• K_c = [O2] 5

For the reaction, CO(g) + Cl2(g) ⇌ COCl₂(g) the K_p/K_c is equal to

• 1/RT

• 1.0

• √RT

• √RT

The equilibrium constant for the reaction N₂(g) + O₂(g) ⇌ 2NO(g) at temperature T is 4×10^-4. The value of K_c for the reaction NO(g) ⇌ 1/2N₂(g) + 1/2O₂(g) at the same temperature.

• 2.5×10²

• 0.02

• 4 x 10^-4

• 4 x 10^-4