Textbook Question
How many bromine atoms are present in 12.8 g of CH2Br2?
Ch.3 - Molecules and Compounds
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 3, Problem 92b
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.
Recommended video:
Guided course
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.
Recommended video:
Guided course
01:16Stoichiometry Concept
Related Practice
Textbook Question
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)
1921
views
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
3869
views
1
comments
Textbook Question
How many fluorine atoms are present in 45.3 g of C2F4?
Textbook Question
Determine the number of moles of hydrogen atoms in each sample. c. 2.4 mol C6H12
1527
views
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
691
views