The equilibrium constant for the reaction
SO₃ (g) $$\leftrightharpoons$$ SO₂ (g) + $$1 \over 2$$ O₂ (g)
is K_c = 4.9 $$\times$$ 10^–2. The value of K_c for the reaction
2SO₂ (g) + O₂ (g) $$\leftrightharpoons$$ 2SO₃ (g) will be :

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 :