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)

The Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables. 

Ideal Gas Law Derivations

Concept #1: The Ideal Gas Law Derivations

Example #1: A sample of sulfur hexachloride gas occupies 8.30 L at 202 ºC. Assuming that the pressure remainsconstant, what temperature (in ºC) is needed to decrease the volume to 5.25 L?

Practice: A sample of nitrogen dioxide gas at 130 ºC and 315 torr occupies a volume of 500 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130 ºC?

Practice: A cylinder with a movable piston contains 0.615 moles of gas and has a volume of 295 mL. What will its volume be if 0.103 moles of gas escaped?

Practice: On most spray cans it is advised to never expose them to fire. A spray can is used until all that remains is the propellant gas, which has a pressure of 1350 torr at 25 ºC. If the can is then thrown into a fire at 455 ºC, what will be the pressure (in torr) in the can?

a) 750 torr

b) 1800 torr

c) 2190 torr

d) 2850 torr

e) 3300 torr