Domanda del libro di testo
What are the empirical formulas of substances with the following mass percent compositions? (b) Ilmenite (a titanium-containing ore): 31.63% O, 31.56% Ti, 36.81% Fe
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Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 3, Problema 89
Ferrocene, a substance proposed for use as a gasoline additive, has the percent composition 5.42% H, 64.56% C, and 30.02% Fe. What is the empirical formula of ferrocene?
Guida verificata passo dopo passo1
Assume you have 100 grams of ferrocene, which allows you to directly convert the percentage of each element to grams: 5.42 g of H, 64.56 g of C, and 30.02 g of Fe.
Convert the mass of each element to moles by dividing by their respective molar masses: \( \text{H: } \frac{5.42 \text{ g}}{1.01 \text{ g/mol}} \), \( \text{C: } \frac{64.56 \text{ g}}{12.01 \text{ g/mol}} \), \( \text{Fe: } \frac{30.02 \text{ g}}{55.85 \text{ g/mol}} \).
Determine the mole ratio of the elements by dividing each element's mole value by the smallest number of moles calculated in the previous step.
Round the mole ratios to the nearest whole number to find the subscripts for each element in the empirical formula.
Write the empirical formula using the whole number mole ratios as subscripts for each element.
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Percent Composition
Percent composition refers to the percentage by mass of each element in a compound. It is calculated by dividing the mass of each element in a sample by the total mass of the compound and multiplying by 100. Understanding percent composition is essential for determining the relative amounts of each element, which is a crucial step in finding the empirical formula.
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Percorso guidato
00:38
Mass Percent Calculation
Empirical Formula
The empirical formula of a compound represents the simplest whole-number ratio of the elements present. It is derived from the percent composition by converting the percentages to moles and then simplifying the mole ratios. This formula provides insight into the basic structure of the compound without detailing the actual number of atoms in a molecule.
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02:26Empirical vs Molecular Formula
Mole Concept
The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number (approximately 6.022 x 10^23) of entities, whether they are atoms, molecules, or ions. This concept is crucial for converting percent composition to moles, which is necessary for calculating the empirical formula.
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Percorso guidato
01:25Mole Concept
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