All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Avogadros hypothesis. At the same volume, pressure, and temperature, samples of different gases have the same number of molecules but different masses.How many moles of gas are in each vessel?

Problem

At the same volume, pressure, and temperature, samples of different gases have the same number of molecules but different masses.  At a volume of 22.4 liters, with a pressure of 1 atmosphere and a temperature of 0 degrees celsius, helium will have a mass of 4.00 grams, diatomic nitrogen will have a mass of 28.0 grams, and methane will have a mass of 16.0 grams.  All three will have a quantity of gas molecules equal to 6.02 times 20^23.
Avogadros hypothesis. At the same volume, pressure, and temperature, samples of different gases have the same number of molecules but different masses.

How many moles of gas are in each vessel?