Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
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: Why are the critical temperature and pressure for H2O so much higher than those for H2S, a related substance?

Solution: Why are the critical temperature and pressure for H2O so much higher than those for H2S, a related substance?

Problem

Why are the critical temperature and pressure for H2O so much higher than those for H2S, a related substance?

Solution
  • Critical temperature and pressure are the temperature and pressure at which a substance may still co-exist in the gaseous and liquid phase. Above the critical temperature, the gas can no longer be liquefied no matter how much pressure is applied.
  • The critical temperature and pressure are influenced by intermolecular forces of attraction (IMFA). The stronger the IMFA, the higher critical temperature and pressure because more energy in needed to vaporize the liquid until critical point.
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