Final answer:
The balanced chemical equation for the preparation of oxygen by heating mercuric oxide is 2HgO(s) -> 2Hg(l) + O2(g). When 1 mole of mercuric oxide is heated, 0.5 moles of oxygen gas are produced. If 10 grams of mercuric oxide are heated, 16 grams of oxygen are produced. The type of reaction that occurs is a decomposition reaction.
Step-by-step explanation:
(a) The balanced chemical equation for the preparation of oxygen by heating mercuric oxide, HgO, is:
2HgO(s) → 2Hg(l) + O²(g)
(b) According to the balanced equation, 2 moles of mercuric oxide produce 1 mole of oxygen gas. Therefore, 1 mole of mercuric oxide will produce 0.5 moles of oxygen gas.
(c) The molar mass of mercuric oxide (HgO) is 216.59 g/mol. Using the molar ratio from part (b), we can calculate the mass of oxygen produced when 1 mole of mercuric oxide decomposes:
0.5 moles of O² * (32.00 g/mol) = 16.00 g
So, when 10 grams of mercuric oxide are heated, the mass of oxygen produced is 16 grams.
(d) The type of reaction that occurs when mercuric oxide is heated to produce oxygen is a decomposition reaction, where a single compound breaks down into two or more simpler substances.