Solid mercury(II) oxide decomposes when heated to produce liquid mercury and oxygen.
2HgO(s) $\leftrightarrows$ 2Hg(l) + O₂(g)
An amount of mercury(II) oxide is placed in a vessel at a particular temperature and allowed to reach equilibrium. How could the amount of liquid mercury in the vessel be increased?
I. Adding more mercury(II) oxide.
II. Removing some oxygen.
III. Increasing the volume of the vessel.

Question

Solid mercury(II) oxide decomposes when heated to produce liquid mercury and oxygen.
2HgO(s)

\leftrightarrows

2Hg(l) + O₂(g)
An amount of mercury(II) oxide is placed in a vessel at a particular temperature and allowed to reach equilibrium. How could the amount of liquid mercury in the vessel be increased?
I. Adding more mercury(II) oxide.
II. Removing some oxygen.
III. Increasing the volume of the vessel.

Quizplus · Accepted Answer

Removing some oxygen will shift the equilibrium to the right, producing more liquid mercury. Increasing the volume of the vessel will decrease the pressure, also shifting the equilibrium to the right, according to Le Chatelier's principle.

Solid Mercury(II) Oxide Decomposes When Heated to Produce Liquid Mercury ⇆\leftrightarrows⇆

Solid Mercury(II) Oxide Decomposes When Heated to Produce Liquid Mercury $\leftrightarrows$