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: A form of Boyle’s law is PV = k (at constant T and n). Table 8-1 contains actual data from pressure–volume experiments conducted by Robert Boyle. The value of k in most experiments is 14.1 x 102 in Hg • in3. Express k in units of atm • L. In Example 8-3, k was determined for NH3 at various pressures and volumes. Give some reasons why the k values differ so dramatically between Example 8-3 and Table 8-1.

Problem

A form of Boyle’s law is PV = k (at constant T and n). Table 8-1 contains actual data from pressure–volume experiments conducted by Robert Boyle. The value of k in most experiments is 14.1 x 102 in Hg • in3. Express k in units of atm • L. In Example 8-3, k was determined for NH3 at various pressures and volumes. Give some reasons why the k values differ so dramatically between Example 8-3 and Table 8-1.