1 mol of PCl₅, kept in a closed container of volume 1 dm³ and was allowed to attain equilibrium at 423 K. Calculate the equilibrium composition of reaction mixture. (The K_c value for PCl₅ dissociation at 423 K is 2)

1 mol of CH₄, 1 mole of CS₂ and 2 mol of H₂S are 2 mol of H₂ are mixed in a 500 ml flask. The equilibrium constant for the reaction K_C = 4 x 10^–2 mol² lit^–2. In which direction will the reaction proceed to reach equilibrium ?

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

A sealed container was filled with 1 mol of A₂ (g), 1 mol B₂ (g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 1 for the reaction
A₂ (g) + B₂ (g) ⇌ 2AB (g)

The partial pressure of carbon dioxide in the reaction
CaCO₃ (s) ⇌ CaO (s) + CO₂(g) is 1.017 × 10^–3 atm at 500⁰C. Calculate K_p at 600⁰C for the reaction. ΔH for the reaction is 181 KJ mol^–1 and does not change in the given range of temperature.