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

Slides:



Advertisements
Similar presentations
Aim: What is thermochemistry?. Law of Conservation of Energy In any chemical or physical process, energy is neither created nor destroyed. There are different.
Advertisements

Ch. 11 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.
Energy in Chemical & 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.
Thermal Energy A. Temperature & Heat 1. Temperature is related to the average kinetic energy of the particles in a substance.
Chapter 17 Thermochemistry.
Thermochemistry and Energy Water freezing and boiling at the same time, really?!
Unit 10 Thermochemistry.
Daily Science April 13 What is STP? Use the reaction shown below to answer the questions:  CO + NO  N 2 + CO 2 Balance the equation If 42.7 g of CO is.
Thermal Energy.
Energy  Cooks the food we eat  Propels vehicles that transport us  Allows photosynthesis to occur to start the food chain  Energy from burning fuels.
QUIZ ON ACIDS & BASES AT THE BEGINNING OF CLASS. TAKE A FEW MINUTES AND STUDY!! PICK UP THE TWO HANDOUTS.
Thermochemistry Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.
Thermochemistry the study of the transfer of energy between reacting chemicals and their surroundings.
Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state.
Thermochemistry.
THERMO- CHEMISTRY Thermochemistry Study of the heat changes that occur during a chemical reaction.
Ch. 15: Energy and Chemical Change
1 Thermochemistry -Energy of Chemical Reactions -OR- -The study of heat changes that occur during chemical reactions and physical changes of state.
Thermochemistry Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.
ENERGY AND CHEMICAL CHANGE Chapter 15. ENERGY ENERGY: -the ability to do work or produce heat. 2 different forms: potential and kinetic -Measured in.
 Energy – the ability to do work or produce heat ◦ Kinetic energy – energy of motion ◦ Potential energy – stored energy  Chemical potential energy –
Energy & Heat Crystal Gray Joshua Osborne Samuel Anum Maurice Torrance.
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.
Thermochemistry. Energy Energy – the ability to do _________ or produce _________ Exists in 2 forms:  Kinetic energy – energy of _________  Potential.
What is Energy? energy (def)-the capacity of an object to do work or produce heat Ch. 10 is concerned with 2 types of energy: kinetic and potential.
What’s the MATTER: Specific Heat of Matter. Matter, Specific Heat of Matter At the conclusion of our time together, you should be able to: 1. Define specific.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Thermochemistry Virtually every chemical reaction is accompanied.
Specific Heat Capacity Every substance has it’s own specific heat because it has a different arrangement of atoms SubstanceSpecific Heat (J/g°C) Water4.18.
Kinetic Energy Energy an object possesses when in motion. Law of Conservation of Energy – in any physical or chemical change, energy can change form,
Energy Ability to “do work” or produce a change. Forms: potential energy and kinetic energy Types: mechanical, electrical, nuclear, solar, chemical, etc.
CHAPTER 10 Reaction Energy Visual Concepts Heat Chapter 10.
Energy. What is Energy? Energy is the ability to do work or produce heat Energy exists in two basic forms –Potential Energy: energy due to the composition.
Ch. 17 Thermochemistry and Energy A liquid freezing and boiling at the same time, really?!
TO LIVE IS THE RAREST THING IN THE WORLD. MOST JUST EXIST. THAT IS ALL.
Unit 10 ~ Thermochemistry (Chapter 10) And you Introduction and Definitions (Section 10.1) Thermochemistry is the study of heat energy changes in.
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.
Thermal Energy Temperature & Heat 1. Temperature is related to the average kinetic energy of the particles in a substance.
Review  Endothermic reactions _________________ energy causing the q and ∆H to be ______________.  Exothermic reactions ___________________ energy causing.
Specific Heat Quantity of energy needed to increase the temperature of one gram of a substance by one degree Celsius/Kelvin Every substance has its own.
Ch.1: Matter and Change Introduction to Thermochemistry.
Thermochemistry: Energy and Heat The Nature of Energy u Energy is the ability to do work or produce heat. u It exists in two basic forms, potential energy.
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
Aim: What is thermochemistry?
Chapter 17 Thermochemistry.
Chapter 16: Energy and Chemical Change
Discovery Lab - Energy.
Bellringer 11/30 Determine the Kelvin temperature required for mole of gas to fill a balloon to 1.20 L under atm pressure.
Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state.
Thermochemistry Study of transfers of energy as heat that accompany chemical rxns and physical changes Part 1.
Reaction Energy Exothermic reaction of Thermite.
Ch. 16 Energy + Chemical Change
Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.
Chapter 16 Thermochemistry
Thermochemistry Lecture 1.
Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state.
Ch.17: Reaction Energy and Reaction Kinetics
Energy 16.1.
Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.
Chapter 16 Preview Objectives Thermochemistry Heat and Temperature
Thermochemistry.
Presentation transcript:

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

Energy Heat (q) = –Form of energy –always flows from a warmer object to a cooler object Law of Conservation of Energy – Energy is neither created nor destroyed

Energy Kinetic energy – in a chemical reaction temperature is the determining factor The higher the temperature…the faster the particles move…the higher the average kinetic energy Temperature is a measure of the average kinetic energy Kelvin scale: 0 K = -273 °C Potential energy – in a chemical reaction deals with the types of atoms & what bonds they form

Heat (q) The SI unit is the joule 1 Cal (food) = 1000 cal (science) = 1 kcal 1 cal = J

Specific Heat (C) Specific Heat (C) – the amount of heat required to raise 1 gram of a substance by 1  C Specific heat is an intensive property, Every substance has its own specific heat Ex. Water = 4.18 J/(g x ºC) Glass = 0.50 J/(g x ºC)

Specific Heat Units for C = J / g ● ºC (joules per gram degree Celsius) Equation for Specific Heat: C = q / (m Δ T) This equation can be rearranged to solve for heat (q) q= CmΔT C = specific heat; q = heat; m = mass and ΔT = change in temperature

Specific Heat A 10.0 g sample of iron changes temperature from 25.0  C to 50.4  C while releasing 114 joules of heat. Calculate the specific heat of iron.

Example C= q/ (m∆T) C=114 J/ (10.0 g x 25.4°C) c = J/g  C

Another example If the temperature of 34.4 g of ethanol increases from 25.0  C to 78.8  C how much heat will be absorbed if the specific heat of the ethanol is 2.44 J/g  C

Another example First, rearrange the specific heat formula to solve for heat q = Cm  T q = (2.44 J/g°C)(34.4g)(78.8°C – 25.0°C) q = 4520 J

Yet another example 4.50 g of a gold nugget absorbs 276 J of heat. What is the final temperature of the gold if the initial temperature was 25.0  C & the specific heat of the gold is 0.129J/g  C

Yet another example C= q/ (m∆T); rearrange to find ∆T = q / (C x m) ∆T = 276 J / (.129 J/g°C x 4.50 g)  T = 475  C  T = Tf-Ti 475 = Tf - 25 Tf = 500  C

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

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