Aim: I.O.SWBAT: 1)Define vapor pressure 2)Interpret phase change diagrams 3)Describe critical temperature and pressure 4)Draw a phase change diagram MOTIVATION:

Slides:



Advertisements
Similar presentations
Question Can water boil at room temperature?. How do We Interpret Phase Diagrams?
Advertisements

Chapter 11 Liquids and Intermolecular Forces
States of Matter The fundamental difference between states of matter is the distance between particles. © 2009, Prentice-Hall, Inc.
Section 12.4: Phase Changes
What is a Phase? A phase is a homogeneous, physically distinct, and mechanically separable portion of matter. It is uniform throughout, both in chemical.
States of matter Solids and Liquids
Chapter 11 1 Ch 11 Page 467. STATES OF MATTER CH CH CH 5The internet? Phase Change- The transformation from one phase to another upon the.
Phases of Matter.
Phase Changes Melting Vaporization Condensation Freezing Sublimation.
Chapter 11 Liquids and Intermolecular Forces
States of matter Solids and Liquids 1. Gases, Solids, and Liquids Phase Particle Properties SpacingEnergyMotionVolumeShape Solid Liquid Gas closelowvibrationaldefinite.
Phase Changes Chapter 11. Vaporization An endothermic process in which the intermolecular attractions of a liquid are broken releasing molecules as a.
Intermolecular Forces Chapter 11 Intermolecular Forces, Liquids, and Solids John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice.
Vapor Pressure and Changes of State Heat of vaporization Enthalpy of vaporization energy required to vaporize 1 mole of a liquid at a pressure of 1 atm.
Intermolecular Forces © 2009, Prentice-Hall, Inc. Evaporation, Vapor Pressure, and Intermolecular Forces John D. Bookstaver St. Charles Community College.
Intermolecular Forces Chapter 11 Intermolecular Forces, Liquids, and Solids.
Phase Diagrams Unit # 11.
Vapor Pressure The molecules at the surface can spontaneously go into a gas as KE increases enough to break attractive forces.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.
Phase Changes Vaporization- The process of changing from a liquid to a gas. Endothermic- lower energy liquid goes to a higher energy gas. When this occurs.
Phase Equilibriums.
Copyright 1999, PRENTICE HALLChapter 111 Phase Changes Surface molecules are only attracted inwards towards the bulk molecules. Sublimation: solid  gas.
Vapor Pressure and Boiling Vapor Pressure – the pressure exerted by a vapor in equilibrium with its liquid state. Vapor Pressure – the pressure exerted.
Changes in States of Matter
Liquids and Solids The Condensed States of Matter Chapter 10.2 – 10.3.
NOTES: Relationship Between Gases & Liquids; Phase Changes & Phase Diagrams.
Phase Diagrams Chapter 11. Chemical Systems Undergo three main processes that change their energy –Chemical reactions –Heating/cooling –Phase transitions.
Crystalline solids Same lattice can be used to describe many different designs For designs based on the fcc unit cell: lattice points, empty spaces, edge.
Courtesy: labinitio.com. Vaporization or evaporation: molecules of a liquid escaping the liquid’s surface and forming a gas. Vaporization is endothermic.
Preview Lesson Starter Objectives Changes of State and Equilibrium Equilibrium Vapor Pressure of a Liquid Boiling Freezing and Melting Phase Diagrams Chapter.
The States of Matter States of Matter u There are 4 states of matter. u A solid is a form of matter that has its own definite shape and volume.
The States of Matter The state a substance is in at a particular temperature and pressure depends on two antagonistic entities: 1) The kinetic energy of.
Chapter 11 – Intermolecular Forces, Liquids and Solids Homework: 13, 16, 18, 19, 23, 43, 45, 47, 48, 49, 50, 51, 54, 55, 56.
Phase Diagrams SOLID LIQUID GAS Critical Point Triple Point vaporizationcondensation sublimation deposition melting freezing.
Phase Diagrams and the Equilibrium of Substances 11/3/10 1.
Heating Curves. Energy and Phase Change When adding heat to a solid, energy added increases the temperature and entropy until the melting point is reached.
Phase Changes.
© 2015 Pearson Education, Inc. Chapter 11 Liquids and Intermolecular Forces James F. Kirby Quinnipiac University Hamden, CT Lecture Presentation.
Chapter 10: States of Matter Changes of State. Objectives Explain the relationship between equilibrium and changes of state. Interpret phase diagrams.
Phase Diagrams CHEM HONORS. Kinetic Theory of Matter Kinetic Theory of Matter: molecules are always moving Measure kinetic energy with a thermometer known.
Vapor Pressure. Evaporation u When fastest particles in a sample of liquid escape from the surface of the liquid u During evaporation the slower particles.
Phase Diagrams & Heating Curves
Evaporation Vaporization = conversion of a liquid to a gas or vapor
Intermolecular Forces Chapter 11 Intermolecular Forces and Liquids John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall,
Phase Diagrams AP Chemistry.
Notes 11-3 Obj 11.5, Rubbing alcohol feels cold when it evaporates from the skin due to the fact that rubbing alcohol has: a.an exothermic heat.
What is a Phase diagram? Phase diagram: plot of pressure vs. Temperature summarizing all equilibria between phases. Given a temperature and pressure, phase.
Intermolecular Forces Chapter 11 Intermolecular Forces, Liquids, and Solids John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice.
Phases of Matter. Kinetic Theory All matter is made of atoms and molecules that act like tiny particles. These tiny particles are always in motion. The.
Phase Changes.
11.3 Some Properties of Liquids
and the Equilibrium of Substances
Phases of Matter Particle Nature of Matter and Changes of State 4:19.
Liquids and Solids Changes of State.
Chapter 7 Lesson Starter
Unit 9 States of Matter.
Phase Changes.
Vapor Pressure Vaporization - change from liquid to gas at boiling point. Evaporation - change from liquid to gas below boiling point Heat (or Enthalpy)
Intermolecular Forces, Liquids, and Solids
Possible Changes of State
Phase Diagrams and Vapor Pressure
PHASE DIAGRAMS.
Phase Diagrams: represent phases dependent on pressure and temperature. liquid solid Pressure gas Temperature.
Phase Diagrams: represent phases dependent on pressure and temperature. liquid solid Pressure gas Temperature.
Section 5: Phase Diagrams:
and the Equilibrium of Substances
Phase Diagrams: represent phases dependent on pressure and temperature. liquid solid Pressure gas Temperature.
States of Matter Lesson 4.2
AP Chem Turn in Shaving Cream Lab if you have not done so yet!
Thermochemistry.
Presentation transcript:

Aim: I.O.SWBAT: 1)Define vapor pressure 2)Interpret phase change diagrams 3)Describe critical temperature and pressure 4)Draw a phase change diagram MOTIVATION: What happens ice at -25oC if your add heat to it?

Do-Now: How does the behavior of a liquid in a closed container differ from that in an open one? Vapor: Gas form of a substance that is a solid or a liquid at room temperature.

LIQUID GAS Dynamic equilibrium: Vaporization and condensation occur at the same rate.

As more molecules escape the liquid, the pressure they exert increases. Vapor pressure: partial pressure of the vapor over the liquid measured at equilibrium

At any temperature, some molecules in a liquid have enough energy to escape. As the temperature rises, the fraction of molecules that have enough energy to escape increases.

Boiling point: is the temperature at which the vapor pressure of a liquid equals the surroundings pressure.

Vapor Pressure Curves The normal boiling point is the temperature at which its vapor pressure is 760 torr.

Volatile liquids: Liquids with a high vapor pressure and weak intermolecular forces. (have low boiling points ) Volatility: The tendency of a substance to evaporate easily.

PRACTICE: 1)Why does the vapor pressure of a liquid depend on intermolecular forces? 2)Why does it take longer to hard boil an egg at high elevations? 3)How does a pressure cooker cook food faster?

Do-Now: Complete hand-out.

Phase diagram: Is a graphic representation of the relationships between the physical state of a substance and its pressure and temperature.

The AB line is the liquid-vapor interface. Each point along this line is the boiling point of the substance at that pressure.

Triple point (A): solid, liquid and gas are in nequilibrium. Critical point (B): Beyond this temperature gas cannot be liquefied by increasing pressure.

The AD line is the interface between liquid and solid. The melting point at each pressure can be found along this line.

Below A the substance cannot exist in the liquid state. Along the AC line the solid and gas phases are in equilibrium. (the sublimation point at each pressure is along this line)

Phase Diagram of Water The slope of the solid– liquid line is negative. –As the pressure is increased at a temperature just below the melting point, water goes from a solid to a liquid.

The high critical point of water is due to the strong van der Waals forces between water molecules.

Phase Diagram of Carbon Dioxide Carbon dioxide cannot exist in the liquid state at pressures below 5.11 atm. CO 2 sublimes at normal pressures. Isotherm: constant temperature Isobar: constant pressure

PRACTICE: Complete Hand-Out HW#44