Presentation is loading. Please wait.

Presentation is loading. Please wait.

Thermochemistry Lecture 1.

Published byLoren Underwood Modified over 6 years ago

Similar presentations

Presentation on theme: "Thermochemistry Lecture 1."— Presentation transcript:

1 Thermochemistry Lecture 1

2 Thermochemistry Study of heat changes of chemical reactions and phase changes System: specific part of the universe that contains the reaction or process you are studying Surrounding: everything in universe except the system

3 Energy Ability to do work or produce heat
2 Forms Kinetic Potential Law of Conservation of Energy Energy can be converted from one form to another in a reaction, but it is neither created nor destroyed

4 Heat Symbol : q Energy that is in the process of flowing from a warmer object to cooler object Measured in Joules (J)

5 Specific Heat Amount of heat required to raise the temperature of one gram of that substance by 1°C. Measure of how efficiently that substance absorbs heat (directly proportional) Symbol : c Water = J/g*°C Water has a high specific heat allowing it to absorb or release large quantities of energy

6 Heat Absorbed or Released by objects
The heat absorbed or released by a substance during a change in temperature depends on specific heat, change in temperature and the mass of the substance. q = c*m*ΔT ΔT = final T – initial T

7 Practice Problem If the temperature of a 34.4 g of ethanol increases from 25.0°C to 78.8°C, how much heat has been absorbed by the ethanol? Specific heat of ethanol: 2.48 J/g*°C 4.52*10^3 Joules

8 Measuring heat Calorimetry
Insulated device used for measuring the amount of heat absorbed or released during a chemical or physical process Can be used to calculate the specific heat of an unknown

9 Practice Question If a 50 g unknown metal with a temperature of 115.0°C, is placed in 125 g of 25.6°C water in a foam cup calorimeter and the metal causes the water to raise it’s temperature to 29.3°C, what is the specific heat of the metal? Part 1: solve the heat the water gained Part 2: heat gained by water = heat lost by metal Part 3: Using the change in temperature of the metal = final T of water – initial T of metal Part 1: q=mcT Q = * 125 * ( ) = 1900 J Part 2 1900 J = q(metal) = mcT Part 3 1900 J = 50 g * c * ( ) C= 0.44 J/g*°C

Download ppt "Thermochemistry Lecture 1."

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.

Aim: What is thermochemistry?. Law of Conservation of Energy In any chemical or physical process, energy is neither created nor destroyed. There are different.
Measuring and Using Energy Changes Section 20.2

Measuring and Using Energy Changes Section 20.2
THERMODYNAMICS Courtesy of lab-initio.com. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or.

THERMODYNAMICS Courtesy of lab-initio.com. Definitions #1 Energy: The capacity to do work or produce heat Potential Energy: Energy due to position or.
EQ: Describe the parts and each part’s function in a calorimeter?

EQ: Describe the parts and each part’s function in a calorimeter?
Exothermic and Endothermic Processes Essentially all chemical reactions and changes in physical state involve either: a) release of heat, or b) absorption.

Exothermic and Endothermic Processes Essentially all chemical reactions and changes in physical state involve either: a) release of heat, or b) absorption.
Laboratory 12 CALORIMETRY. Objectives 1.Construct and utilize a coffee cup calorimeter to measure heat changes 2.Determine the heat capacity of a calorimeter.

Laboratory 12 CALORIMETRY. Objectives 1.Construct and utilize a coffee cup calorimeter to measure heat changes 2.Determine the heat capacity of a calorimeter.
Thermochemistry -- The Flow of Energy: Heat -- Thermochemistry: the study of heat changes in chemical reactions Chemical potential energy: energy stored.

Thermochemistry -- The Flow of Energy: Heat -- Thermochemistry: the study of heat changes in chemical reactions Chemical potential energy: energy stored.
Calorimetry Chapter 5. Calorimetry Since we cannot know the exact enthalpy of the reactants and products, we measure  H through calorimetry, the measurement.

Calorimetry Chapter 5. Calorimetry Since we cannot know the exact enthalpy of the reactants and products, we measure  H through calorimetry, the measurement.
Energy in Chemical & Physical Changes

Energy in Chemical & Physical Changes
Energy. Energy – the ability to do work Energy – the ability to do work Kinetic – energy of motion, anything that moves has kinetic energy. Kinetic –

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

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?!

Thermochemistry and Energy Water freezing and boiling at the same time, really?!
Unit 10 Thermochemistry.

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.

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.
Section 15-1 The Nature of Energy Energy is the ability to do work or produce heat.Energy weightless, odorless, tasteless Two forms of energy exist, potential.

Section 15-1 The Nature of Energy Energy is the ability to do work or produce heat.Energy weightless, odorless, tasteless Two forms of energy exist, potential.
A calorimeter is used to measure the amount of heat absorbed or released during a chemical reaction.A calorimeter is used to measure the amount of heat.

A calorimeter is used to measure the amount of heat absorbed or released during a chemical reaction.A calorimeter is used to measure the amount of heat.
QUIZ ON ACIDS & BASES AT THE BEGINNING OF CLASS. TAKE A FEW MINUTES AND STUDY!! PICK UP THE TWO HANDOUTS.

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 Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.
Energy can change form and flow, but it is always conserved. Section 1: Energy K What I Know W What I Want to Find Out L What I Learned.

Energy can change form and flow, but it is always conserved. Section 1: Energy K What I Know W What I Want to Find Out L What I Learned.
Measuring and Using Energy Changes Section 20.2. Main Idea Energy stored in chemical bonds can be converted to other forms and used to meet the needs.

Measuring and Using Energy Changes Section Main Idea Energy stored in chemical bonds can be converted to other forms and used to meet the needs.

Similar presentations

Ads by Google