Textbook Question
An unknown liquid is composed of 34.31% C, 5.28% H, and 60.41% I. The molecular weight found by mass spectrometry is 210.06. What is the molecular formula of the compound?
Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- 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
Chapter 3, Problem 91c
What are the empirical formulas of each of the following substances? (c) Zircon, a mineral from which cubic zirconia is made: 34.91% O, 15.32% Si, 49.77% Zr
Verified step by step guidance1
Convert the percentage of each element to grams, assuming you have 100 grams of the compound. This means you have 34.91 grams of O, 15.32 grams of Si, and 49.77 grams of Zr.
Convert the mass of each element to moles by dividing by their respective molar masses: O (16.00 g/mol), Si (28.09 g/mol), and Zr (91.22 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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Empirical Formula
An empirical formula represents the simplest whole-number ratio of the elements in a compound. It is derived from the percentage composition of each element in the substance, allowing chemists to understand the basic composition without detailing the molecular structure.
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Percentage Composition
Percentage composition refers to the mass percentage of each element in a compound. To find the empirical formula, one must first convert the given percentages into moles, which involves dividing the percentage of each element by its molar mass, thus determining the relative amounts of each element present.
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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 grams and moles, allowing for the calculation of the number of moles of each element in a compound based on its percentage composition, which is essential for deriving the empirical formula.
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Related Practice
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