Consider the reaction

$$\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{l})+3 \mathrm{CQ}_2(\mathrm{~g})$$

In accordance with Le-Chatlier's principle, which of the following will not disturbs the equilibrium?

At $$700 \mathrm{~K}$$, the Equilibrium constant value for the formation of $$\mathrm{HI}$$ from $$\mathrm{H}_2$$ and $$\mathrm{I}_2$$ is 49.0 . 0.7 mole of $$\mathrm{HI}(\mathrm{g})$$ is present at equilibrium. What will be the concentrations of $$\mathrm{H}_2$$ and $$\mathrm{I}_2$$ gases if we initially started with $$\mathrm{HI}(\mathrm{g})$$ and allowed the reaction to reach equilibrium at the same temperature?

$$\mathrm{S}_8$$ on heating at a temperature above $$1000 \mathrm{~K}$$, changes to $$\mathrm{S}_2$$. When 1 mole of $$\mathrm{S}_8$$ is heated above $$1000 \mathrm{~K}$$, the pressure falls by $$32 \%$$ at equilibrium. The equilibrium constant for the conversion is: