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: In any real gas, attractive intermolecular forces reduce pressure to values lower than in an ideal gas.How would you expect the pressure of a gas to change if suddenly the intermolecular forces wer

Problem

A diagram shows that molecules of an ideal gas bounces off the walls of a container, creating a strong force of pressure. But real gas molecules are attracted to each other, lessening the force resulting from collisions with the wall, so that the pressure in that system is much less.
In any real gas, attractive intermolecular forces reduce pressure to values lower than in an ideal gas.

How would you expect the pressure of a gas to change if suddenly the intermolecular forces were repulsive rather than attractive?