Domanda del libro di testo
The compound XCl4 contains 75.0% Cl by mass. What is the element X?
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
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Brown 15th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 48a
Brown 15th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 48aCapitolo 3, Problema 48a
Determine the empirical formulas of the compounds with the following compositions by mass: a. 55.3% K, 14.6% P, and 30.1% O
Guida verificata passo dopo passo1
Convert the percentage of each element to grams, assuming you have 100 grams of the compound. This means you have 55.3 grams of K, 14.6 grams of P, and 30.1 grams of O.
Convert the mass of each element to moles by dividing by their respective molar masses: K (39.10 g/mol), P (30.97 g/mol), and O (16.00 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.
If necessary, multiply the mole ratios by a whole number to get the smallest whole number ratio for each element.
Write the empirical formula using the whole number mole ratios as subscripts for each element.
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Empirical Formula
The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the mass percentages of each element, which are converted into moles to find the ratio. This formula does not provide information about the actual number of atoms in a molecule but rather the relative proportions of each element.
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02:26
Empirical vs Molecular Formula
Mole Concept
The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole corresponds to Avogadro's number, approximately 6.022 x 10²³ entities (atoms, molecules, etc.). To determine the empirical formula, the mass percentages of elements are converted to moles by dividing by their respective atomic masses, allowing for the calculation of the simplest ratio.
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Percorso guidato
01:25Mole Concept
Mass Percent Composition
Mass 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. This information is crucial for determining the empirical formula, as it provides the necessary data to convert to moles and establish the ratios of the elements.
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00:38Mass Percent Calculation
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