Units: g/mL, g/cm3.

Slides:



Advertisements
Similar presentations
Thermochemistry.
Advertisements

Thermochemistry the study of transfers of energy as heat that accompany chemical reactions and physical changes.
Chemistry Ms. Piela  Heat transfers in chemical reactions  Energy  Definition: The capacity to do work or supply heat  Basic Types: Mechanical, Electrical,
 Energy is transferred ◦ Exothermic – heat is released  Heat exits ◦ Endothermic – heat is required or absorbed by reaction  Measure energy in Joules.
Thermochemistry The Basics of Heat Transfer. The Flow of Energy Thermochemistry - concerned with heat changes that occur during chemical reactions.
Rates of Reactions Mr. Skirbst Physical Science Topic 18.
Endothermic/Exothermic Processes & Reactions
ENDOTHERMIC AND EXOTHERMIC REACTIONS. EXOTHERMIC REACTIONS Chemical Reactions that RELEASE heat with the products. You may see an exothermic reaction.
What is the relationship between heat and temperature?
Unit 2 – Matter and Energy Mrs. Callender. Lesson Essential Question: What is Thermochemistry?
Chemical Reactions That Involve Heat Objectives: 1. Describe the difference between exothermic and endothermic reactions. 2. Explain the relationship between.
 All chemical reactions involve energy  Exothermic reactions release energy  Energy will appear on the product side of the equation  Ex. Fast freddie.
Energy Section 3-3 (somewhat). Energy Physical and chemical changes are always accompanied by energy changes. – Released (Exothermic) – Absorbed (Endothermic)
Thermochemistry.
Thermal Energy A. Temperature & Heat 1. Temperature is related to the average kinetic energy of the particles in a substance.
Energy changes in chemical reactions. When the head of a match is struck, energy is released. Some of this energy heats the surroundings and some is released.
Section 1.   Chemical Energy:  Energy that matter possess because of its chemical makeup.  Where does the energy come from?  Movements of the atoms.
Ch. 15: Energy and Chemical Change
Heat and Temperature. The difference Heat – the energy that flows from hot to cold. Measured in Joules (J) or calories (cal). Temperature – measure of.
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.
Measuring Changes of Heat and Temperature over time. “It was the heat of the moment”
THERMOCHEMISTRY Specific Heat Thermochemistry 17.1  Thermochemistry is the study of energy changes (HEAT) that occur during chemical reactions and changes.
Energy Flow. Energy the ability to do work energy has no mass nor volume but is only detected by its effects thermochemistry studies energy changes during.
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.
Kinetic Energy Energy an object possesses when in motion. Law of Conservation of Energy – in any physical or chemical change, energy can change form,
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?
Calories from food Chapter 12. Calories Measurement of the energy content in a substance = heat Calorie = E require to raise the temperature of 1 gram.
 Different substances require different amounts of heat to change their temperature.  Objects that require more energy have a high heat capacity like.
16.1 Thermochemistry. POINT > Define temperature and heat POINT > Define specific heat POINT > Describe enthalpy of reaction POINT > Define enthalpy of.
5.2 Calorimetry and Enthalpy. Measuring Energy Changes Calorimetry is the experimental process used to measure the transfer of thermal energy. – A bomb.
Matter in Motion The molecules that make up matter are in constant motion. These molecules have kinetic energy.
Chemistry Notes Energy and Heat Heat Capacity and Specific Heat.
ENERGY n The ability to do work n remains constant in amount during a chemical or physical change n energy changes occur between the system and the surrounding.
(17.1) Energy Transformations
Chapter 17 Thermochemistry.
Thermo-chemistry.
Specific Heat Calorimetry.
Specific Heat Capacity
Chemical reactions alter arrangements of atoms
Reaction Energy Exothermic reaction of Thermite.
LECTURE 8.4 – CALORIMETRY.
Heat Exchange -Heat ALWAYS travels in the direction of: HOT  COLD
Heat and Endothermic and Exothermic Reactions
Chapter 16 Thermochemistry
Bond Energy and Reaction Energy
Chapter 6: Thermochemistry
Thermodynamics.
Unit 2 Chemistry Lesson 4 Changes in Matter Essential Questions: 1
Thermochemistry.
Chemistry of Life 2.4 Chemical Reactions.
Drill __NaNO3(s) + __H2SO4(l) → __Na2SO4(s) + __HNO3(g)
The Law of Mass Conservation & Energy in Reactions
Thermochemistry.
Thermochemistry.
Thermochemistry Chapter 16.
Warm Up #1 What is a catalyst?
Ch 10 - Energy.
Law of Conservation of Mass
The Flow of Energy.
Units for temperature: Fahrenheit Celsius Kelvins
Energy and Chemical Changes
Thermochemistry.
Energy in Chemical Reactions
Exothermic and Endothermic changes
Reaction Energy.
Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.
Heat and Temperature.
Heat and Energy! Created by Educational Technology Network
Presentation transcript:

Units: g/mL, g/cm3

Energy

the part of the universe under consideration SYSTEM the part of the universe under consideration (ex. An atom or a beaker with chemicals)

Energy in a reaction is released (gets hot) EXOTHERMIC Energy in a reaction is released (gets hot)

Energy in a reaction is absorbed (gets cold) ENDOTHERMIC Energy in a reaction is absorbed (gets cold)

Energy transferred as a result of a temperature difference HEAT Energy transferred as a result of a temperature difference (Symbol = q)

JOULE SI unit on energy (Symbol = J)

Specific Heat (Cp) The heat required to raise the temperature of 1 gram of substance by 1°C. Unit = J / (g)(°C)

Every material has its own specific heat (see Appendix Table A-3)

q = (m)(ΔT)(Cp) Heat lost or gained = mass * change in temp * specific heat of a substance

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2025 SlidePlayer.com. Inc. All rights reserved.