Equilibrium Tes...

Direction (Q. Nos. 1-12) This section contains 12 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.
 

Q.Conversion factor for converting partial pressures (in K_p) to active masses (in K_c) is

For which of the following reactions does the equilibrium constant depends on the unit of concentration?

The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,

 is 1.3 x 106 and that for 

is 6.5 x 10^-16 (when each species is expressed in terms of partial pressure).
For the reaction,

equilibrium constant is

For the following gaseous phase equilibrium,

K_p is found to be equal to K_x (K_x is equilibrium constant when concentration are taken in terms of mole fraction. This is attained when pressure is 

For the reaction in equilibrium, A B

Thus, K is

For the following equilibrium, N₂O₄ (g) 2NO₂(g)

K_p = K_C. This is attained when

 is a gaseous phase equilibrium reaction taking place at 400 K in a 5 L flask. For this 

A sample of pure PCI₅(g)was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of PCI₅ was found to be 0.05 mol L^-1.

Thus, [PCI₃] and [Cl₂](in mol L^-1)at equilibrium are

Ag⁺(aq)+NH₃(aq) [Ag(NH₃)(aq)]⁺ ; K, = 3.5x 10^-3
[Ag(NH₃)]⁺ (aq)+NH₃(aq) [Ag(NH₃)₂]²⁺(aq); K₂ = 1.7x 10^-3
Formation constant of [Ag(NH₃)₂]⁺(aq) is

For the reversible reaction, 
at 500° C, the value of K_p is 1.44x 10^-5, when partial pressure is measured in atmosphere. The corresponding value of K_c with concentration in mol L^-1 is

[IITJEE 2000]

For the reaction, 
if K_p = K_c (RT)^X, when the symbols have usual meaning, the value of x is (assuming ideality)

[jee Main 2014]

Given that for the equilibrium constants of two reactions,

areK₁ and K₂. Equilibrium constant k₃ of the following reaction in terms of k₁, and K₂.