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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

Chemistry Gas Laws

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Sections
Pressure Units
Manometer
Partial Pressure
The Ideal Gas Law
Standard Temperature and Pressure
Effusion
Root Mean Square Speed
Kinetic Molecular Theory
Van der Waals Equation
Velocity Distribution
End of Chapter 5 Problems
Additional Practice
Chemistry Gas Laws
Ideal Gas Law Density
Ideal Gas Law Molar Mass
Gas Stoichiometry
Collecting Gas Over Water
Kinetic Energy of Gases
Additional Guides
Ideal Gas Law
Boyle's Law
Combined Gas Law
Additional Practice

Solution: A 12 Liter tank contains helium gas pressurized to 160 atm.How many 3-liter balloons could the 12 Liter helium tank fill?(Keep in mind that an "exhausted" helium tank is not empty. In other words, onc

Solution: A 12 Liter tank contains helium gas pressurized to 160 atm.How many 3-liter balloons could the 12 Liter helium tank fill?(Keep in mind that an "exhausted" helium tank is not empty. In other words, onc

Problem

A 12 Liter tank contains helium gas pressurized to 160 atm.

How many 3-liter balloons could the 12 Liter helium tank fill?

(Keep in mind that an "exhausted" helium tank is not empty. In other words, once the gas inside the tank reaches atmospheric pressure, it will no longer be able to fill balloons.)

Solution

Recall: The ideal gas law is given by the equation: PV = nRT

At constant temperature and moles of gas:

The equation P1V1 = P2V2 is Boyle's Law, which states that the pressure of a certain amount of gas at a certain temperature is inversely proportional to its volume, i.e. the pressure decreases as volume increases.

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