Textbook Question
(a) What are the mole fractions of H2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
Ch.10 - Gases
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 10, Problem 72a1
(a) What are the mole fractions of O2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
Verified step by step guidance1
Calculate the number of moles of each gas using their respective molar masses: O_2 (32.00 \(\text{ g/mol}\)), N_2 (28.02 \(\text{ g/mol}\)), and H_2 (2.02 \(\text{ g/mol}\)).
Find the total number of moles in the mixture by summing the moles of O_2, N_2, and H_2.
Determine the mole fraction of O_2 by dividing the moles of O_2 by the total moles in the mixture.
Express the mole fraction of O_2 as a decimal.
Ensure that the sum of the mole fractions of all gases in the mixture equals 1 as a check for accuracy.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 10²³) of entities, whether they are atoms, molecules, or ions. This concept is essential for converting grams of a substance to moles, which is necessary for calculating mole fractions.
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Mole Concept
Mole Fraction
Mole fraction is a way of expressing the concentration of a component in a mixture. It is defined as the ratio of the number of moles of a specific component to the total number of moles of all components in the mixture. Mole fractions are dimensionless and provide a useful means of comparing the relative amounts of different substances in a mixture.
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Calculating 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 atoms in a molecule. Knowing the molar mass of each gas in the mixture is crucial for converting the given masses of O₂, N₂, and H₂ into moles, which is a necessary step for determining their mole fractions.
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Related Practice
Textbook Question
A rigid vessel containing a 3:1 mol ratio of carbon dioxideand water vapor is held at 200 °C where it has a total pressureof 202.7 kPa. If the vessel is cooled to 10 °C so that all of thewater vapor condenses, what is the pressure of carbon dioxide?Neglect the volume of the liquid water that forms on cooling.
Textbook Question
(a) What are the mole fractions of N2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
Textbook Question
(b) What is the partial pressure in atm of each component of this mixture if its held in a 15.50-L vessel at 15 °C?
Textbook Question
At an underwater depth of 100 m, the pressure is 1.106 MPa.What should the partial pressure of oxygen be in the divinggas for the mole fraction of oxygen in the mixture to be 0.21,the same as in air?
Textbook Question
A quantity of N2 gas originally held at 531.96 kPa pressurein a 1.00-L container at 26 °C is transferred to a 12.5-L containerat 20 °C. A quantity of O2 gas originally at 531.96 kPaand 26 °C in a 5.00-L container is transferred to this samecontainer. What is the total pressure in the new container?