Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) ⇌ [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value of equilibrium constant.

The following water gas shift reaction is an important industrial process for the production of hydrogen gas.
CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)
At a given temperature K_p = 2.7. If 0.13 mol of CO, 0.56 mol of water, 0.78 mol of CO₂ and 0.28 mol of H₂ are introduced into a 2 L flask, and find out in which direction must the reaction proceed to reach equilibrium

The equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) ⇌ 2NO₂(g);
\(\Delta \mathrm{H}_{\mathrm{f}}^{\circ}=57.32 \mathrm{KJmol}^{-1}\)
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100^o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

At particular temperature K_C = 4 x 10^–2 for the reaction
H₂S(g) ⇌ H₂(g) + ½ S₂(g)
Calculate KC for each of the following reaction
i) 2H₂S (g) ⇌ 2H₂ (g) + S₂ (g)
ii) 3H₂S (g) ⇌ 3H₂ (g) + 3/2 S₂(g)

The equilibrium for the dissociation of XY₂ is given as,
2XY₂ (g) ⇌ 2XY (g) + Y₂(g)
if the degree of dissociation x is so small compared to one. Show that 2 K_P = PX₃ where P is the total pressure and K_P is the dissociation equilibrium constant of XY₂.