Textbook Question
How many fluorine atoms are present in 5.85 g of C2F4?
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Ch.3 - Molecules, Compounds & Chemical Equations
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 3, Problem 84b
Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). b. CFCl3
Verified step by step guidance1
Determine the molar mass of CFCl_3 by adding the atomic masses of its constituent elements: C, F, and Cl.
Calculate the mass percentage of chlorine in CFCl_3 by dividing the total mass of chlorine atoms by the molar mass of CFCl_3 and multiplying by 100.
Convert the given mass of CFCl_3 from kilograms to grams for easier calculation.
Use the mass percentage of chlorine to find the mass of chlorine in the given mass of CFCl_3 by multiplying the mass percentage by the total mass of CFCl_3.
Convert the mass of chlorine from grams back to kilograms to match the desired units for the final answer.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. For chlorofluorocarbon CFCl3, the molar mass can be determined by adding the atomic masses of carbon (C), fluorine (F), and chlorine (Cl) based on their respective quantities in the formula.
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02:11
Molar Mass Concept
Mass Percentage
Mass percentage is a way to express the concentration of an element in a compound, calculated as the mass of the element divided by the total mass of the compound, multiplied by 100. This concept is essential for determining how much of a specific element, like chlorine, is present in a given mass of a compound, such as CFCl3.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the substances involved in chemical reactions. It allows chemists to calculate the amounts of reactants and products based on balanced chemical equations. In this context, stoichiometry helps in determining the mass of chlorine in a specified mass of CFCl3 by using the compound's molar mass and mass percentage.
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01:16Stoichiometry Concept
Related Practice
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Calculate mass (in grams) of sodium in 8.5 g of each sodium containing food additive. a. NaCl (table salt) b. Na3PO4 (sodium phosphate) c. NaC7H5O2 (sodium benzoate) d. Na2C6H6O7 (sodium hydrogen citrate)
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Textbook Question
Determine the number of moles of oxygen atoms in each sample. a. 4.88 mol H2O2 b. 2.15 mol N2O c. 0.0237 mol H2CO3 d. 24.1 mol CO2
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Textbook Question
Determine the number of moles of hydrogen atoms in each sample. c. 2.4 mol C6H12
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Textbook Question
A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. a. 1.245 g Ni, 5.381 g I
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How many bromine atoms are present in 35.2 g of CH2Br2?
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