11.6 NOTES Phase Diagrams.

Slides:



Advertisements
Similar presentations
PHASE CHANGES SECTION 3.3.
Advertisements

I. Kinetic Molecular Theory KMT
Section 12.4: Phase Changes
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.
Phases of Matter.
Phase Changes Section 17.3 in YOUR book.
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.
Liquids and Solids The Condensed States of Matter Chapter 10.2 – 10.3.
10.4  Phase – any part of a system with uniform composition and properties.  Condensation – gas changes to a liquid  Molecules of liquid can evaporate.
Chp Phase Changes Pg Characteristics of Phase Changes  When at least two states of a substance are present, each state is described as.
Chapter 10, Section 4  Changes of State. Phase  Any part of a system that has uniform composition and properties.
The universe is made up of: The system – the thing that you are studying The surroundings- everything else.
Section 3.3 Phase Changes.
Liquids & Vapor Pressure. Vapor Pressure (VP) = Pressure exerted by vapor over its liquid How is vapor pressure affected by temperature? higher the temperature,
Phase Diagrams & Heating Curves
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. Phase Change Phase Change: Reversible physical change that occurs when substance changes from one state to another Energy is either released.
States of Matter Phase Change. Water Water exists on our planet in three states. Ice, water, and water vapor What causes water to be in one phase or another?
WATER CYCLE ASSESSMENT NUMBER TWO REVIEW GOAL: WE WILL UNDERSTAND NEW WATER CYCLE VOCABULARY TERMS AND REVIEW THE WATER CYCLE PROCESS.
Vapor and it Pressure. Vapor Definition: Gas phase of a substance that is normally a liquid at room temperature. Some particles have enough KE to “escape”
Phase Changes Phase change – a reversible physical change that happens when a substance changes from one state of matter to another. 6 Common Phase Changes.
Phase Changes Notes 3.3.
PHASE CHANGES Each state of matter is called a PHASE
definite volume definite shape regular geometric pattern
States of Matter I. Describing the States of Matter:
PHASE CHANGES SECTION 3.3.
Phases of Matter Particle Nature of Matter and Changes of State 4:19.
Liquids and Solids Changes of State.
A large iceberg contains enough fresh water to supply millions of people with water for a year. As it moves into warmer areas, the ice changes to liquid.
Chapter 7 Lesson Starter
REVIEW.
Think First Retake tests after school TODAY!
Daily Science February 18
Section 2 Changes of State.
5 Changes of States of Matter
Heating Curves & Phase Change Diagrams
Phase Changes.
Liquids & Vapor Pressure
States of Matter I. Describing the States of Matter:
Possible Changes of State
Physical Phase Changes
Phase Diagrams and Vapor Pressure
Changes of State BELLWORK-name the following state changes:
Ch. 13 – States of Matter III. Phase Changes (p. 425 – 429)
Phase Diagrams plot of P vs.T showing states of matter
Changes of State Chapter 3 Section 3.
Liquids & Vapor Pressure
Liquids & Solids Changes of State.
PHASE CHANGES SECTION 3.3.
Chapter 3 Section 3 Notes Phase Changes.
Changes of State Section 4.3.
The Nature of Energy 1.
Phase Changes (Section 3.3)
States of Matter Lesson 4.2
AP Chem Turn in Shaving Cream Lab if you have not done so yet!
Chapter 13 Phase Changes Notes #8b.
Changes in states of matter pt.1
Changes of State Textbook pages
Changes in states of matter pt.1
Chp Phase Changes Pg
3.3 Physical Changes due to particle energy
I can describe what happens during melting and freezing
Phase Changes.
States of Matter I. Describing the States of Matter:
Phases of Matter.
Changes in states of matter pt.1
Change of State.
Liquids & Vapor Pressure
Change of State.
Presentation transcript:

11.6 NOTES Phase Diagrams

IV. Phase Changes A. Phase changes that require energy Endothermic 1. Melting phase change from a liquid to a solid - amount of energy to melt one mole of solid depends on the strength of the forces keeping the particles together in the solid - MP = temp at which solid and liquid phases of a substance coexist;

2. Vaporization process by which a liquid changes to a gas or vapor; phase change from a liquid to a gas - difference b/t evaporation and BP = evaporation occurs at all temps and only at the surface of the liquid while boiling occurs at a specific temp and pressure and occurs throughout the liquid body sweat – requires energy to evaporate liquid, when liquid does evaporate it takes (heat) energy with it;

Vapor Pressure - pressure exerted by a vapor over a liquid an increase in temp would increase vapor pressure vapor – gas phase of a substance that is normally a liquid at room temp; a.k.a. equilibrium vapor pressure Boiling point - the temp @ which the vapor pressure of a liquid equals the atmospheric (external) pressure; if walls of container are smooth, temp of liquid may get higher than that of BP, use boiling chip to prevent spattering; vacuum pump demo

3. Sublimation solid directly to gas; I2 and CO2 (solids) sublime @ room temp - examples – moth balls and solid air freshners;

B. Phase changes that release energy Exothermic 1. Condensation process by which gas becomes a liquid - clouds form when a layers of air high above the Earth’s surface cool - clouds = small H2O droplets; rain = large droplets

2. Deposition change from gas to solid; snowflakes and frost; H2O(g) to solid; 3. Freezing change from liquid to solid; FP and MP are the same temp;  

C. Phase diagrams - phase is dependent on temp and pressure - T and P can have opposite effects on a substance - i.e. increase temp, cause L G while increase pressure causes G  L

- plot of pressure vs. temperature shows in which phase a substance exists under different conditions of temp. and pressure - any point on the line will represent gas-liquid boundary/solid-liquid boundary/gas-solid boundary - gas/liquid boundary represents Boiling Point at that pressure - solid/liquid boundary represents Melting Point at that pressure

if line is to the right represents the solid is more dense than the liquid and the MP increases as pressure increases (most substances) - if line is to the left like water, represents solid is less dense than liquid and MP decreases with pressure - if start at high P, water will go from liquid to solid to gas; why freeze drying works - place fresh veggies in freezer  1st water is frozen and then as pressure drops ice quickly sublimes to lock in freshness and taste;

Phase diagram for water Phase diagram for carbon dioxide

- Triple point point at which all 3 phases occur simultaneously with the 6 phase changes; if in closed system would be very odd looking; - Critical temperature and pressure point at which no matter how much pressure is applied, gas will not liquefy - corresponds to pressure as well; lower the critical temp, harder a substance is to liquefy;