Clutch Prep is now a part of Pearson
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
Pressure Units
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Mole Fraction
Partial Pressure
The Ideal Gas Law: Molar Mass
The Ideal Gas Law: Density
Gas Stoichiometry
Standard Temperature and Pressure
Root Mean Square Speed
Kinetic Energy of Gases
Maxwell-Boltzmann Distribution
Velocity Distributions
Kinetic Molecular Theory
Van der Waals Equation
Additional Guides
Boyle's Law (IGNORE)
Charles Law (IGNORE)
Ideal Gas Law (IGNORE)
Jules Bruno

Boyle’s Law, also known as Mariotte’s Law or the Boyle-Mariotte Law, states that pressure and volume are inversely proportional as long as moles (n) and temperature (T) are held constant. 

Boyle’s Law 

In a closed container, pressure represents the downward force applied to it while the volume represents the free space inside of it. According to Boyle’s Law, as the pressure on a container increases then the inside volume will decrease and vice-versa. 

Boyle-Law-Compression-ExpansionInversion Relationship of Pressure & Volume

This opposing relationship can be illustrated by the following pressure-volume graph: 

Isothermal-Process-PV-plot-GraphPV Graph

The inverse relationship between pressure and volume at a constant mass for a gas at a fixed temperature is illustrated by the expression: 

Boyle-Law-ExpressionBoyle's Law Expression

Boyle’s Law Formula

The Ideal Gas Law is presented as: 

Ideal-Gas-LawIdeal Gas Law

If moles (n) and temperature (T) are held constant then the formula simplifies into: 

cconstant-Ideal-Gas-Law-ConstantIdeal Gas Law (Simplified)

In this form k represents our constant and when dealing with two sets of data for pressure and volume we obtain the Boyle’s Law Formula as: 

Boyle-Law-Formula-EquationBoyle's Law Formula

Now let’s use it in a practice problem. 

PRACTICE: A gas occupies 4.23 L at 2.25 atm. What is the volume at 3.46 atm?

STEP 1: Identify the variables given. 

Given-Variables-Boyle-LawIdentifying given variables (Boyle's Law)

STEP 2: Isolate the missing variable for the second volume (V2). 

Solving-Missing-Variable-V2Solving missing variable (V2)

Beyond Boyle’s Law

Boyle’s Law represents one of the Simple Gas Laws besides Charles Law, Avogadro’s Law and Gay-Lussac’s Law. In order to understand non-ideal gases we must examine the kinetic theory of gases and the Van der Waals equation

Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.