How many grams of HgO would you need to heat if you wanted to prepare 0.0155 mol of O2 according to the equation in Problem 10.70?

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Identify the balanced chemical equation for the decomposition of mercury(II) oxide (HgO). The reaction is: 2 HgO(s) \rightarrow 2 Hg(l) + O_2(g).

Determine the molar ratio between HgO and O_2 from the balanced equation. From the equation, 2 moles of HgO produce 1 mole of O_2.

Calculate the moles of HgO needed to produce 0.0155 moles of O_2 using the molar ratio. Since 2 moles of HgO produce 1 mole of O_2, you need 2 \times 0.0155 moles of HgO.

Find the molar mass of HgO. The molar mass of HgO is the sum of the atomic masses of Hg (200.59 g/mol) and O (16.00 g/mol), which is 216.59 g/mol.

Calculate the mass of HgO required by multiplying the moles of HgO by its molar mass.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate how much of a substance is needed or produced based on the balanced chemical equation. In this case, understanding the stoichiometric ratios from the decomposition of HgO to O2 is essential for determining the mass of HgO required.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between moles and grams in stoichiometric calculations. For HgO, knowing its molar mass allows us to calculate how many grams correspond to the moles needed to produce the desired amount of O2.

Decomposition Reaction

A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler products. In the case of HgO, heating it causes it to decompose into mercury (Hg) and oxygen gas (O2). Understanding this reaction is vital for determining how many moles of HgO are needed to produce the specified moles of O2.

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