The exothermic formation of ClF₃ is represented by the equation:
Cl₂ (g) + 3F₂ (g) $$\leftrightharpoons$$ 2ClF₃ (g); $$\Delta H$$ = -329 kJ
Which of the following will increase the quantity of ClF₃ in an equilibrium mixture of Cl₂, F₂ and ClF₃?

For the reaction 2NO₂ (g) $$\leftrightharpoons$$ 2NO (g) + O₂ (g), (K_c = 1.8 $$\times$$ 10^-6 at 184^oC) (R = 0.0831 kJ/(mol. K))
When K_p and K_c are compared at 184^oC , it is found that :

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. Pressure. Ammonium hydrogen sulphide decomposes to yield NH₃ and H₂S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH₄HS decomposition at this temperature is :

What is the equilibrium expression for the reaction
P₄ (s) + 5O₂ $$\leftrightharpoons$$ P₄O₁₀ (s)?