Final answer:
Mercury(II) oxide decomposes when heated, yielding mercury and oxygen. This reaction exemplifies a decomposition reaction and involves careful handling due to toxicity. Understanding the stoichiometry of the reaction is essential for predicting product amounts.
Step-by-step explanation:
When mercury(II) oxide (HgO) is exposed to temperatures above 500°C, it undergoes a decomposition reaction. This reaction, which is indicative of a color change from red to silvery, results in the formation of liquid mercury and oxygen gas (O₂). Decomposition reactions are a type of chemical reaction where a compound is broken down into simpler substances. This specific reaction of HgO is noteworthy not only for its visually observable change but also for the need to handle mercury compounds with care due to their toxicity.
In the classroom setting, calculating the moles of HgO that decompose, the consequent moles of O₂ produced, and the volume of O₂ at specified conditions of temperature and pressure could be an illustrative application of this reaction. Understanding the stoichiometry involved in this reaction is crucial for students who study chemistry, both at the high school and collegiate levels. Determining the stoichiometry helps in predicting the amounts of products formed from a given amount of reactant, which is essential in practical chemical applications and experiments.