Energy Unit 1. States of Matter Changing State of Matter.

Slides:

Advertisements

Similar presentations

Thermochemistry the study of transfers of energy as heat that accompany chemical reactions and physical changes.

Advertisements

Thermochemistry The Basics of Heat Transfer. The Flow of Energy Thermochemistry - concerned with heat changes that occur during chemical reactions.

Ch. 11 Thermochemistry.

Thermal Force Unit 1.4.

UNIT 3 ENERGY AND STATES 1. The State of Matter of a substance depends on several things Attraction between particles called IMF or Inter- Molecular Forces.

Everything that is not matter.. Think of all the ways this word is used… o.0?

Unit 09 Thermochemistry.

Chapter 6: Thermal Energy. LEARNING GOALS  Define temperature.  Explain how thermal energy depends on temperature.  Explain how thermal energy and.

Thermal energy and Heat. Thermal energy Thermal energy is the total kinetic energy of all particles in a substance Measured in joules (J) This is not.

Chapter 6: Thermochemistry

Energy Kinetic energy = energy of motion. Energy Potential energy = stored energy 1. energy of position due to gravity.

Reaction Energy and Reaction Kinetics Thermochemistry.

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Unit 9 Thermochemistry Cartoon courtesy of NearingZero.net.

Section 10.2 The Flow of Energy 1.To understand how heat energy flows and how it is measured 2.To understand how substances differ in their capacity to.

Energy. Energy – the ability to do work Energy – the ability to do work Kinetic – energy of motion, anything that moves has kinetic energy. Kinetic –

Thermochemistry Heat a form of energy. can be transferred between samples heat flows from matter at a higher temperature to matter at a lower temperature.

Energy and Heat 15.1 and 15.2 (pgs. 516 – 528). Main Idea… Energy can change form and flow, but it is always conserved The enthalpy change for a reaction.

Thermochemistry and Energy Water freezing and boiling at the same time, really?!

What does temperature measure? What does pressure measure?

Thermochemistry. A look at the new unit Chapter 11: Thermochemistry –Endothermic –Exothermic –Changes in states of water Chapter 19.3 and 19.4: Spontaniety.

Thermochemistry: The heat energy of chemical reactions Enthalpy is the amount of ________ transferred during a reaction. The symbol for the change in enthalpy.

Play the PowerPoint for narration

Chapter 17 pgs q= m x c x T  This is the equation for all Thermochemistry problems  The Q is heat values in either calories or joules (4.18.

Thermal Energy.

Chapter 5 Energy.

Energy A Give and Take The Nature of Energy Energy: the ability to do work or produce heat Potential energy (store energy): energy due to position.

Ch. 21 Temperature, Heat, and Expansion. Question to the class: Discuss with your neighbor, in what terms have we discussed energy so far? – What equations.

Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state.

Thermochemistry.

Ch. 15: Energy and Chemical Change

Thermochemistry: The heat energy of chemical reactions

Quantifying Heat The Math!.

Ch 13: Solids and Liquids Ch 13 begins with notes from Ch 3.6 and 3.7 on Energy, Temperature and Heat. We did not do these sections when in Ch 3 as the.

The Flow of Energy-Heat Energy and Heat. Energy Energy is weightless, odorless, and tasteless Gasoline is an example of chemical potential energy Different.

Specific Heat Capacity. deals with heat changes that occur during chemical reactions deals with heat changes that occur during chemical reactions Heat.

Phases of Matter and Heat Transfer. Matter Video on the discovery of the nucleus.

Chem10 Topic 01 - Thermochemistry Science 10 CT01D01.

Heat: Lesson 4 Heat vs. Temperature. What happens to the movement of molecules as they’re heated? /energy-forms-and-changeshttp://phet.colorado.edu/en/simulation.

Thermodynamics X Unit 9. Energy: Basic Principles  Thermodynamics – the study of energy changes  Energy – the ability to do work or produce heat Note:

Quantifying Heat The Math!. What is HEAT?  It’s the flow of energy due to a difference in temperature.  From a higher temperature (higher kinetic energy)

Thermodynamics X Unit 9. Energy: Basic Principles  Thermodynamics – the study of energy changes  Energy – the ability to do work or produce heat Kinetic.

Chemistry I Chapter 10 Review Calorie – energy needed to raise temp. of 1g of water 1 o C Energy – ability to do work or produce heat Endothermic – energy.

Properties of Matter Specific Heat. Couple of Terms: Heat may be defined as energy in transit from a high temperature object to a lower temperature object.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Thermochemistry Virtually every chemical reaction is accompanied.

Thermochemistry. Chemical reactions involve changes in energy Breaking bonds releases energy Forming bonds requires energy The energy involved in chemistry.

CHAPTER 10 Reaction Energy Visual Concepts Heat Chapter 10.

1 Energy in Chemical Reactions EQ: How is energy calculated? How are reaction determined to be endo/exothermic?

Ch. 17 Thermochemistry and Energy A liquid freezing and boiling at the same time, really?!

Energy change that occurs during a chemical reaction and/or changes in state.

TO LIVE IS THE RAREST THING IN THE WORLD. MOST JUST EXIST. THAT IS ALL.

Section 10.2 The Flow of Energy 1.To convert between different energy units. 2.To understand the concept of heat capacity. 3.To solve problems using heat.

Thermodynamics Chemistry. Thermodynamics The study of energy changes in physical and chemical processes.

Just What Is It How Can We Define Energy The capacity to do work Or the ability to cause a change to occur.

Review  Endothermic reactions _________________ energy causing the q and ∆H to be ______________.  Exothermic reactions ___________________ energy causing.

Matter in Motion The molecules that make up matter are in constant motion. These molecules have kinetic energy.

Chapter 17 Thermochemistry.

Thermochemistry.

Temperature, Heat, and Expansion

Endothermic & Exothermic Reactions

Thermochemistry Study of transfers of energy as heat that accompany chemical rxns and physical changes Part 1.

Thermochemistry Chapter 10.

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Chapter 16 Thermochemistry

Thermochemistry Feeling hot, hot, hot.

DO NOW: (back of Notes) On a cold winter’s day you open the door to your house. Are you letting the cold in, or the heat out? How is the amount of calories.

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Presentation transcript:

Energy Unit 1

States of Matter

Changing State of Matter

Changing States of Matter  In order to go from 1 state of matter to another, it involves energy (usually heat energy- enthalpy)  You are either removing the energy or adding more energy

How does heat move? From areas of higher temperature to lower temperature! Endothermic Processes  Occur when heat is added to the system  Examples  Cooking  Evaporation  Instant cold packs Exothermic Processes  Occur when heat is given off by the system  Examples  Instant heat packs  Nuclear fission  Candle burning

Exothermic or Endothermic?

What is HEAT ?  It’s the flow of energy due to a difference in temperature.  From a higher temperature (higher kinetic energy) to a lower temperature (less kinetic energy)  THERE IS NO SUCH THING AS COLD!  It’s just the absence of heat!  What is temperature ?  It’s the average amount of kinetic energy a substance has from its moving atoms/ molecules  Kinetic energy is the energy of motion!

Equation q = mCΔT heat energy – measured in joules (J) mass - measured in grams (g) heat capacity – how much heat a substance can hold, measured in joules/gram  degrees Celsius change in temperature, measured in °C ΔT = T final – T initial

Units for heat (q)  Most food tells us the amount of energy in units of Calories....  Calories are kilocalories ( 1 Cal = 1000cal )  The SI unit for energy is Joules (J)  1 cal = J  Let’s do some quick conversions.

How can you tell if a process is endothermic or exothermic? Endothermic  q is a positive number  Why?  The final temperature is higher than the initial temperature- we added heat to the system.  ΔT = T final – T initial Exothermic  q is a negative number  Why?  The final temperature is lower than the initial temperature- heat was given off from the system.  ΔT = T final – T initial Let’s solve some problems!