Preview Lesson Starter Objectives Changes of State and Equilibrium Equilibrium Vapor Pressure of a Liquid Boiling Freezing and Melting Phase Diagrams Chapter.

Slides:



Advertisements
Similar presentations
Gases, Liquids and Solids
Advertisements

Phase Changes “It’s just a phase”.
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.
Chapter 13 Notes Sub day Pre Ap students- copy down these notes for Chapter 13. There are two diagrams included. I encourage you to copy these.
Liquids and Solids Changes of State.
Changes of State Matter on Earth can exist in any of these states – gas, liquid, or solid – and can change from one state to another. Listed below are.
Student will learn: 1. to read Phase diagrams 2. math calculations of energy for melting, freezing, vaporization, condensing or raising temperature of.
Why did you not smell the odor of the vapor immediately?
Chapter 10 Preview Lesson Starter Objectives
Phase Changes Chapter 11. Vaporization An endothermic process in which the intermolecular attractions of a liquid are broken releasing molecules as a.
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:
Chapter 10 Preview Lesson Starter Objectives
Chapter 12 Liquids and Solids.
Tuesday, Dec. 3 rd : “A” Day Wednesday, Dec. 4 th : “B” Day (early out) Agenda  Homework Questions/collect (pg. 398: 1-3, 6-9)  Sec quiz: “Energy.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.
Kinetic Energy, Temperature, Phase Changes Chapter 13 Concepts.
The universe is made up of: The system – the thing that you are studying The surroundings- everything else.
A change in state is called a phase change Evaporation is the change in state from liquid to gas Sublimation is the change from solid to gas Both deal.
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.
Phase Change: solid to liquid Melting water Most solids shrink in size when frozen. What substance is an exception and actually expands?
The Nature of Matter. Liquids The ability of gases and liquids to flow allows then to conform to the shape of their containers. Liquids are much more.
Liquids and Solids The Condensed States of Matter Chapter 10.2 – 10.3.
The Kinetic-Molecular Theory of Gases
Chapter 10. The kinetic-molecular theory is based on the idea that particles of matter are always in motion. used to explain the properties of solids,
Liquid-Vapor Equilibrium Section 17.1 (AHL). Vaporization You have a container with a volatile liquid in the bottom Molecules of the liquid will escape.
Phase Diagrams Chapter 11. Chemical Systems Undergo three main processes that change their energy –Chemical reactions –Heating/cooling –Phase transitions.
Chapter 13: States of Matter
Chapter 12 Liquids and Solids Definitions!!!!  Fluid- a substance that can flow and therefore take the shape of its container.  Liquids and Gases.
10.4  Phase – any part of a system with uniform composition and properties.  Condensation – gas changes to a liquid  Molecules of liquid can evaporate.
Physical Science Mr. Moss RHS.  When 2 states are present at the same time, we describe each as a phase.  Here, we see 2 phases of water: ◦ Solid Phase.
Phase Changes Bubble, bubble, toil and trouble....
Courtesy: labinitio.com. Vaporization or evaporation: molecules of a liquid escaping the liquid’s surface and forming a gas. Vaporization is endothermic.
Chapter 10, Section 4  Changes of State. Phase  Any part of a system that has uniform composition and properties.
Phase Diagrams and the Equilibrium of Substances 11/3/10 1.
Section 3.3 Phase Changes.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of GasesThe Kinetic-Molecular Theory.
The kinetic-molecular theory is based on the idea that particles of matter are always in motion. The theory can be used to explain the properties of solids,
Chapter 10: States of Matter Changes of State. Objectives Explain the relationship between equilibrium and changes of state. Interpret phase diagrams.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION Chapter 10 Liquids and Solids.
Evaporation Vaporization = conversion of a liquid to a gas or vapor
Equilibrium Of phases!. Equilibrium Definition: situation where two changes are occurring at equal rates in a closed system Closed system: energy can.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of GasesThe Kinetic-Molecular Theory.
Chemistry Kinetic Molecular Theory States of Matter Chapter 15.
In covalent solids, atoms are held together in an extensive three- dimensional network entirely by covalent bonds. Types of solids 12.4.
13.2 The Nature of Liquids> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 13 States of Matter 13.1 The Nature.
Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of GasesThe Kinetic-Molecular Theory.
Energy/Phases of Matter /Equilibrium Review Game
11.3 Some Properties of Liquids
and the Equilibrium of Substances
Section 10.4.
Liquids and Solids Changes of State.
Chapter 7 Lesson Starter
Heating Curves & Phase Change Diagrams
The Kinetic-Molecular Theory of Gases
Changes of State 10.4.
Changes of State.
Properties of Liquids The attraction between liquid particles is caused by the intermolecular forces: London dispersion forces dipole-dipole forces hydrogen.
Possible Changes of State
Changes of State Chapter 10 Section 4.
Changes of State Section 10.4.
Liquids and Solids Chapter 12.
Heating Curves & Phase Change Diagrams
and the Equilibrium of Substances
Changes of State Chapter 10 Section 4.
Possible Changes of State
Chapter 13 Phase Changes Notes #8b.
Liquids and Solids Chapter 12.
Presentation transcript:

Preview Lesson Starter Objectives Changes of State and Equilibrium Equilibrium Vapor Pressure of a Liquid Boiling Freezing and Melting Phase Diagrams Chapter 10 Section 4 Changes of State

Lesson Starter Why does the balloon inflate after the solid dry ice is added? The solid CO 2 sublimes to form CO 2 gas. The gas occupies more volume than the solid. Section 4 Changes of State Chapter 10

Objectives Explain the relationship between equilibrium and changes of state. Interpret phase diagrams. Explain what is meant by equilibrium vapor pressure. Describe the processes of boiling, freezing, melting, and sublimation. Section 4 Changes of State Chapter 10

Possible Changes of State Section 4 Changes of State Chapter 10

Section 4 Changes of State Mercury in Three States Chapter 10

Changes of State and Equilibrium A phase is any part of a system that has uniform composition and properties. Condensation is the process by which a gas changes to a liquid. A gas in contact with its liquid or solid phase is often called a vapor. Equilibrium is a dynamic condition in which two opposing changes occur at equal rates in a closed system. Section 4 Changes of State Chapter 10

Click below to watch the Visual Concept. Visual Concept Chapter 10 Equilibrium Section 4 Changes of State

Changes of State and Equilibrium, continued Eventually, in a closed system, the rate of condensation equals the rate of evaporation, and a state of equilibrium is established. Section 4 Changes of State Chapter 10

Section 4 Changes of State Liquid-Vapor Equilibrium System Chapter 10

Equilibrium Vapor Pressure of a Liquid Vapor molecules in equilibrium with a liquid in a closed system exert a pressure proportional to the concentration of molecules in the vapor phase. The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature is called the equilibrium vapor pressure of the liquid. The equilibrium vapor pressure increases with increasing temperature. Increasing the temperature of a liquid increases the average kinetic energy of the liquid’s molecules. Section 4 Changes of State Chapter 10

Click below to watch the Visual Concept. Visual Concept Chapter 10 Section 4 Changes of State Equilibrium and Vapor Pressure

Section 4 Changes of State Measuring the Vapor Pressure of a Liquid Chapter 10

Click below to watch the Visual Concept. Visual Concept Chapter 10 Section 4 Changes of State Factors Affecting Equilibrium

Equilibrium Vapor Pressure of a Liquid, continued Every liquid has a specific equilibrium vapor pressure at a given temperature. All liquids have characteristic forces of attraction between their particles. Volatile liquids are liquids that evaporate readily. They have relatively weak forces of attraction between their particles. example: ether Section 4 Changes of State Chapter 10

Equilibrium Vapor Pressure of a Liquid, continued Nonvolatile liquids do not evaporate readily. They have relatively strong attractive forces between their particles. example: molten ionic compounds Section 4 Changes of State Chapter 10

Click below to watch the Visual Concept. Visual Concept Chapter 10 Section 4 Changes of State Comparing Volatile and Nonvolatile Liquids

Boiling Boiling is the conversion of a liquid to a vapor within the liquid as well as at its surface. The boiling point of a liquid is the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure. The lower the atmospheric pressure is, the lower the boiling point is. Section 4 Changes of State Chapter 10

Boiling, continued At the boiling point, all of the energy absorbed is used to evaporate the liquid, and the temperature remains constant as long as the pressure does not change. If the pressure above the liquid being heated is increased, the temperature of the liquid will rise until the vapor pressure equals the new pressure and the liquid boils once again. Section 4 Changes of State Chapter 10

Boiling, continued The normal boiling point of a liquid is the boiling point at normal atmospheric pressure (1 atm, 760 torr, or kPa). The normal boiling point of water is exactly 100°C. Section 4 Changes of State Chapter 10

Boiling, continued Energy and Boiling Energy must be added continuously in order to keep a liquid boiling The temperature at the boiling point remains constant despite the continuous addition of energy. The added energy is used to overcome the attractive forces between molecules of the liquid during the liquid-to-gas change and is stored in the vapor as potential energy. Section 4 Changes of State Chapter 10

Boiling, continued Molar Enthalpy of Vaporization The amount of energy as heat that is needed to vaporize one mole of liquid at the liquid’s boiling point at constant pressure is called the liquid’s molar enthalpy of vaporization, ∆H v. The magnitude of the molar enthalpy of vaporization is a measure of the attraction between particles of the liquid. The stronger this attraction is, the higher molar enthalpy of vaporization. Section 4 Changes of State Chapter 10

Boiling, continued Molar Enthalpy of Vaporization, continued Each liquid has a characteristic molar enthalpy of vaporization. Water has an unusually high molar enthalpy of vaporization due to hydrogen bonding in liquid water. Section 4 Changes of State Chapter 10

Freezing and Melting The physical change of a liquid to a solid is called freezing. Freezing involves a loss of energy in the form of heat by the liquid. liquid solid + energy Section 4 Changes of State Chapter 10 In the case of a pure crystalline substance, this change occurs at constant temperature.

Freezing and Melting, continued The normal freezing point is the temperature at which the solid and liquid are in equilibrium at 1 atm (760 torr, or kPa) pressure. At the freezing point, particles of the liquid and the solid have the same average kinetic energy. Melting, the reverse of freezing, also occurs at constant temperature. solid + energy liquid Section 4 Changes of State Chapter 10

Freezing and Melting, continued At equilibrium, melting and freezing proceed at equal rates. solid + energy liquid Section 4 Changes of State Chapter 10 At normal atmospheric pressure, the temperature of a system containing ice and liquid water will remain at 0.°C as long as both ice and water are present. Only after all the ice has melted will the addition of energy increase the temperature of the system.

Freezing and Melting, continued Molar Enthalpy of Fusion The amount of energy as heat required to melt one mole of solid at the solid’s melting point is the solid’s molar enthalpy of fusion, ∆H f. The magnitude of the molar enthalpy of fusion depends on the attraction between the solid particles. Section 4 Changes of State Chapter 10

Freezing and Melting, continued Sublimation and Deposition At sufficiently low temperature and pressure conditions, a liquid cannot exist. Under such conditions, a solid substance exists in equilibrium with its vapor instead of its liquid. solid + energy vapor Section 4 Changes of State Chapter 10 The change of state from a solid directly to a gas is known as sublimation. The reverse process is called deposition, the change of state from a gas directly to a solid.

Click below to watch the Visual Concept. Visual Concept Chapter 10 Section 4 Changes of State Comparing Sublimation and Deposition

Phase Diagrams A phase diagram is a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist. The triple point of a substance indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium. The critical point of a substance indicates the critical temperature and critical pressure. Section 4 Changes of State Chapter 10

Phase Diagrams The critical temperature (t c ) is the temperature above which the substance cannot exist in the liquid state. Above this temperature, water cannot be liquefied, no matter how much pressure is applied. The critical pressure (P c ) is the lowest pressure at which the substance can exist as a liquid at the critical temperature. Section 4 Changes of State Chapter 10

Click below to watch the Visual Concept. Visual Concept Chapter 10 Section 4 Changes of State Phase Diagram

Phase Diagram for Water Section 4 Changes of State Chapter 10

Phase Diagram for CO2 Section 4 Changes of State Chapter 10

Changes of State Section 4 Changes of State Chapter 10