how-does-increasing-the-pressure-by-decreasing-the-volume-shift-the-equilibrium-

Question

How does increasing the pressure (decreasing the volume) shift the equilibrium of the reaction of uranium with fluorine gas?

U(s) + 3 F₂(g) → UF₆(g) ΔH = −513.24 kcal/mol (−2147.4 kJ/mol)

Accepted Answer

Increasing the pressure of the reaction shifts the equilibrium forward and favors the formation of the product.

Answer

Increasing the pressure of the reaction shifts the equilibrium backward and favors the formation of the product.

Answer

Increasing the pressure of the reaction shifts the equilibrium backward and favors the formation of the reactant.

Answer

Increasing the pressure of the reaction shifts the equilibrium forward and favors the formation of the reactant.

How does increasing the pressure (decreasing the volume) shift the equilibrium of the reaction of uranium with fluorine gas? U(s) + 3 F2(g) → UF6(g) ΔH = −513.24 kcal/mol (−2147.4 kJ/mol)