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: Calculate the pressure (atm) that CCl4 will exert at 43 °C if 1.20 mol occupies 33.5 L, assuming that Part A  CCl4 obeys the ideal-gas equation: Part B  CCl4 obeys the van der Waals equation. (Values

Solution: Calculate the pressure (atm) that CCl4 will exert at 43 °C if 1.20 mol occupies 33.5 L, assuming that Part A  CCl4 obeys the ideal-gas equation: Part B  CCl4 obeys the van der Waals equation. (Values

Problem

Calculate the pressure (atm) that CCl4 will exert at 43 °C if 1.20 mol occupies 33.5 L, assuming that 

Part A  CCl4 obeys the ideal-gas equation: 


Part B  CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are a = 20.4, b = 0.1383.)