Use representations [A] through [I] in Figure P 3.10 to answer questions a-f. a. Which two compo

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Use representations [A] through [I] in Figure P 3.10 to...

Use representations $[\mathrm{A}]$ through $[\mathrm{I}]$ in Figure $\mathrm{P} 3.10$ to answer questions a-f. a. Which two compounds have the same empirical formula? b. Which compound has a molecular mass of 180 amu? c. Which compound might have a molar mass of $180 \mathrm{g} ?$ d. Which compound has the largest percent oxygen by mass? e. The mass of one gold bar in [D] is 12.4 kg. The mass of one silver bar in $[\mathrm{E}]$ is $31 \mathrm{kg} .$ Which contains more atoms - the gold bar or the silver bar? f. When completely combusted, which compound will produce more moles of carbon dioxide- -benzene [A] or table sugar [C]? (IMAGES CAN'T COPY)

Use representations $[\mathrm{A}]$ through $[\mathrm{I}]$ in Figure $\mathrm{P} 3.10$ to answer questions a-f.
a. Which two compounds have the same empirical formula?
b. Which compound has a molecular mass of 180 amu?
c. Which compound might have a molar mass of $180 \mathrm{g} ?$
d. Which compound has the largest percent oxygen by mass?
e. The mass of one gold bar in [D] is 12.4 kg. The mass of one silver bar in $[\mathrm{E}]$ is $31 \mathrm{kg} .$ Which contains more atoms - the gold bar or the silver bar?
f. When completely combusted, which compound will produce more moles of carbon dioxide- -benzene [A] or table sugar [C]?
(IMAGES CAN'T COPY)

Key Concepts

Combustion Stoichiometry

Combustion stoichiometry involves the quantitative analysis of the products formed when a compound is burned completely (such as carbon dioxide and water). By using balanced chemical equations and the mole ratios of reactants to products, one can determine the relative amounts of products generated, which is vital for comparing the outcomes of combustion reactions.

Mole Concept and Atomic Counting

The mole concept provides a link between the mass of a substance and the number of constituent particles it contains, using Avogadro’s number. This concept is essential for converting grams to moles and for determining the number of atoms or molecules in a given sample, which is key in quantitative chemical analysis.

Percent Composition

Percent composition quantifies the contribution of each element to the overall mass of a compound. Calculated by dividing the mass of each individual element by the compound's total molecular mass and multiplying by 100, it is an important diagnostic tool for analyzing the makeup of a substance.

Molecular Mass/Molar Mass

Molecular mass (in amu) and molar mass (in g/mol) describe the total mass of all atoms in one molecule of a compound. This concept is fundamental for identifying and comparing substances based on their mass, and it is crucial when converting between the mass of a compound and the number of moles.

Empirical Formula

An empirical formula represents the simplest whole-number ratio of the elements in a compound. It is used to compare compounds and determine if different molecular formulas have the same basic elemental proportions without considering the actual number of atoms present in a molecule.

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