When mercury(II) oxide, a red crystalline solid, is heated, it decomposes to form liquid mercury and oxygen gas, according to the following equation: ___HgO(s) $\rightarrow$ ___Hg(l) + ___O₂(g)(unbalanced) Balance the equation and determine the mass of mercury that should be formed when 15.6 g of HgO is heated.

Question

Quizplus · Accepted Answer

The balanced equation is 2HgO(s) → 2Hg(l) + O2(g). The molar mass of HgO is 216.59 g/mol, and the molar mass of Hg is 200.59 g/mol. From 15.6 g of HgO, the mass of Hg formed is (15.6 g / 216.59 g/mol) * 200.59 g/mol = 14.4 g.

When Mercury(II) Oxide, a Red Crystalline Solid, Is Heated, It →\rightarrow→

When Mercury(II) Oxide, a Red Crystalline Solid, Is Heated, It $\rightarrow$