Chapter 3 Matter and Energy

Slides:

Advertisements

Similar presentations

1 Chapter 9 Energy and States of Matter 9.6 Changes of State Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.

Advertisements

HEAT EQUATION (in Table T)

1 Chapter 2Energy and Matter 2.4 Specific Heat. 2 Specific heat is different for different substances. is the amount of heat that raises the temperature.

1 Chapter 2Energy and Matter 2.4 Specific Heat. 2 Specific heat is different for different substances. is the amount of heat that raises the temperature.

1 Chapter 2Energy and Matter 2.4 Specific Heat. 2 Specific heat is different for different substances. is the amount of heat that raises the temperature.

 Energy is transferred ◦ Exothermic – heat is released  Heat exits ◦ Endothermic – heat is required or absorbed by reaction  Measure energy in Joules.

How many Joules of energy are required to raise the temperature of 75 g of water from 20.0 o C to 70.0 o C? Heat =75 g x 50.0 o C x 4.18 J/g o C Heat=

Specific Heat Pre – Lab. Specific Heat Different substances require different amounts of heat to change their temperature. In general the specific heat.

Thermochemistry -- The Flow of Energy: Heat -- Thermochemistry: the study of heat changes in chemical reactions Chemical potential energy: energy stored.

General, Organic, and Biological ChemistryCopyright © 2010 Pearson Education, Inc.1 Specific Heat.

THERMODYMANICS Thermodynamics is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

General, Organic, and Biological ChemistryCopyright © 2010 Pearson Education, Inc. Heat Review A. When you touch ice, heat is transferred from 1) your.

Specific Heat Review Cp = q/(m)(Δt).

Chapter 2 Energy and Matter

THERMODYNAMICS: MATH PRESENTATION. EXAMPLE 1: What quantity of heat is required to raise the temperature of 450 grams of water from 15°C to 85°C? The.

1 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Chapter 3 Matter and Energy 3.5 Specific Heat.

1 Temperature and Heat Temperature is the measurement of the avg. KE of the molecules in a material. Heat is the transfer of KE from one material to.

Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Chapter 2 Matter.

Specific Heat mC  T. Specific Heat The amount of heat energy a material requires to raise its temperature is a characteristic that can be used to identify.

Thermal Energy A. Temperature & Heat 1. Temperature is related to the average kinetic energy of the particles in a substance.

Thermodynamics Ch 10 Energy Sections Thermodynamics The 1st Law of Thermodynamics The Law of Conservation of Energy is also known as The 1st.

ENERGY CALCULATION PRACTICE UNIT 3. HOW MUCH ENERGY IS REQUIRED TO HEAT 200 GRAMS OF WATER FROM 25˚C TO 125˚C? HOW MUCH ENERGY IS RELEASED WHEN COOLING.

Thermochemistry Heat Symbol: q Energy that transfers from one object to another NOT TEMPERATURE!!!!!! Observable temperature is caused by heat.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 10 Structures of Solids and Liquids 10.5 Changes of State.

THERMODYMANICS Thermodynamics is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

 Chapter 2Energy and Matter 2.4 Specific Heat Copyright © 2009 by Pearson Education, Inc.

Temperature(“Degree of hotness”) - is the distribution of energy through the molecules. - related to the motion (speed) of molecules. Heat ≠ Temperature.

Reaction Energy and Reaction Kinetics Chapter 17 Notes.

Energy (nrg) How energy changes the physical state of matter & energy involved in chemical 

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 10 Structures of Solids and Liquids 10.5 Changes of State.

Heat and Temperature. The difference Heat – the energy that flows from hot to cold. Measured in Joules (J) or calories (cal). Temperature – measure of.

General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 2.6 Energy and Nutrition Chapter 2 Energy and Matter © 2013 Pearson Education,

Specific Heat Capacity Weather Unit – Science 10.

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

Thermochemical Calculations

1 Temperature and Heat Temperature is the measurement of the avg. KE of the molecules in a material. Heat is the transfer of KE from one material to.

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.

Specific Heat & Phase Changes. Specific Heat ____________ (c) – the amount of heat required to raise the temperature of 1 g of a substance 1 °C The units.

General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 2.5 Specific Heat Chapter 2 Energy and Matter © 2013 Pearson Education, Inc.

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.

Thermodynamics The study of the changes of heat in chemical reactions.

Thermochemistry -- The Flow of Energy: Heat --. Water Constants Solid 7.9 Liquid Gas 8.5.

CHAPTER 10 Reaction Energy Visual Concepts Heat Chapter 10.

Thermodynamics Practice. Heat Absorbed/Released 1.How many joules of heat are needed to raise the temperature of 10.0 g of magnesium from 22°C to 55°C,

Specific Heat Practice. Gold has a specific heat of J/(g°C). How many joules of heat energy are required to raise the temperature of 15 grams of.

Energy exits in two basic forms, ____________________ and ____________________ energy.

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.

Worksheet Chapter Key. 1. Which substance must have more energy removed from it to undergo a ten degree temperature drop? One with a low specific.

Thermal Energy Temperature & Heat 1. Temperature is related to the average kinetic energy of the particles in a substance.

Unit 12 Study session. Practice Specific heat capacity (J/g o C) Initial temperature Final temperature A1540 B1550 C1560 Which metal has the highest specific.

Heat energy is measured in units called joules or calories. 1 calorie is the amount of heat energy needed to raise the temperature of 1.0 g (mL) of water.

Chapter 3 Lecture Basic Chemistry Fourth Edition Chapter 3 Matter and Energy 3.5 Specific Heat Learning Goal Calculate specific heat. © 2014 Pearson Education,

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.

 Different substances require different amounts of heat to change their temperature.  Objects that require more energy have a high heat capacity like.

Thermochemistry Specific Heat.

WS: Calorimetry Problems

Honors Chemistry Podcast 2.3 Joule Problems Q = mc  T.

Energy transfer varies from reaction to reaction.

3.6 Specific Heat The high specific heat of water keeps temperature more moderate in summer and winter. Learning Goal Use specific heat to calculate.

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

Thermochemical Calculations

Thermochemistry Specific Heat.

Energy Content in Foods

Energy Measuring Heat Calorimetry

THERMOCHEMISTRY Thermochemistry is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

SPECIFIC HEAT q = s x m x DT

Chapter 16 Thermochemistry

Chapter 2 Energy and Matter

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

Presentation transcript:

Chapter 3 Matter and Energy 3.5 Specific Heat Learning Goal Calculate specific heat. © 2014 Pearson Education, Inc.

is different for different substances Specific Heat Specific heat is different for different substances is the amount of heat, in joules or calories, needed to change the temperature of 1 g of a substance by 1 ° C in the SI system has units of J/g ° C in the metric system has units of cal/g ° C © 2014 Pearson Education, Inc.

Calculating Specific Heat To calculate the specific heat (SH) of a substance we measure the heat (q) in joules (J), the mass (m) in grams, and the temperature change, which is written as ΔT. For example, the specific heat of water is

Specific Heat of Some Substances

Specific Heat of Liquid Water A large mass of water near a coastal city can absorb or release five times the energy absorbed or released by the same amount of rock near an inland city.

Guide to Calculating Specific Heat

Learning Check What is the specific heat of a metal if 24.8 g of the metal absorbs 275 J of energy and the temperature rises from 20.2 ° C to 24.5 ° C?

Solution What is the specific heat of a metal if 24.8 g of the metal absorbs 275 J of energy and the temperature rises from 20.2 ° C to 24.5 ° C? Step 1 Given 24.8 g, 275 J, ΔT = 4.3 ° C Need J/g ° C Step 2 Write the relationship for specific heat.

Solution What is the specific heat of a metal if 24.8 g of the metal absorbs 275 J of energy and the temperature rises from 20.2 ° C to 24.5 ° C? Step 3 Substitute the given values into equation.

Heat Equation from Specific Heat Rearranging the specific heat expression gives the heat equation.

Heat Equation from Specific Heat The amount of heat lost or gained by a substance is calculated from the following equation q = m × ΔT × SH where m represents the mass of substance (g) the temperature change is represented by (ΔT) the specific heat, (SH) of the substance is given in units of (J/g ° C)

Guide to Calculations Using Specific Heat

Sample Problem, Using SH A layer of copper (Cu) on a pan has a mass of 135 g. How much heat (kJ) is needed to raise the temperature of the copper from 26 ° C to 328 ° C? (The specific heat of Cu is 0.385 J/g ° C.) Step 1 Given 135 g, 26 ° C to 328 ° C, SH = 0.385 J/g ° C Need joules

Sample Problem, Using SH A layer of copper (Cu) on a pan has a mass of 135 g. How much heat (kJ) is needed to raise the temperature of the copper from 26 ° C to 328 ° C? (The specific heat of Cu is 0.385 J/g ° C.) Step 2 Calculate the temperature change. ΔT = 328 ° C – 26 ° C = 302 ° C Step 3 Write the heat equation. q = m × ΔT × SH(Cu)

Sample Problem, Using SH A layer of copper (Cu) on a pan has a mass of 135 g. How much heat (kJ) is needed to raise the temperature of the copper from 26 ° C to 328 ° C? (The specific heat of Cu is 0.385 J/g ° C.) Step 4 Substitute in values and solve.

Learning Check How many kilojoules are needed to raise the temperature of 325 g of water from 15.0 ° C to 77.0 °C? A. 20.4 kJ B. 77.7 kJ C. 84.3 kJ

Solution How many kilojoules are needed to raise the temperature of 325 g of water from 15.0 ° C to 77.0 ° C? C. 84.3 kJ Step 1 Given 325 g water SH(water) = 4.184 J/g ° C 15.0 ° C to 77.0 ° C Need kilojoules

Solution How many kilojoules are needed to raise the temperature of 325 g of water from 15.0 °C to 77.0 °C? C. 84.3 kJ Step 2 Calculate the temperature change. ΔT = 77.0 °C – 15.0 °C = 62.0 °C Step 3 Write the heat equation. q = m × ΔT × SH(water)

Solution How many kilojoules are needed to raise the temperature of 325 g of water from 15.0 °C to 77.0 °C? C. 84.3 kJ Step 4 Substitute in values and solve.

Calculating Heat Loss A 225-g sample of hot tea cools from 74.6 °C to 22.4 °C. How much heat, in kilojoules, is lost, assuming that tea has the same specific heat as water? Step 1 Given 225 g tea (water) SH(water) = 4.184 J/g °C 74.6 °C to 22.4 °C Need kilojoules

Calculating Heat Loss A 225-g sample of hot tea cools from 74.6 °C to 22.4 °C. How much heat, in kilojoules, is lost, assuming that tea has the same specific heat as water? Step 2 Calculate the temperature change. ΔT = 22.4 °C – 74.6 °C = -52.2 °C Step 3 Write the heat equation. q = m × ΔT × SH(water)

Calculating Heat Loss A 225-g sample of hot tea cools from 74.6 ° C to 22.4 ° C. How much heat, in kilojoules, is lost, assuming that tea has the same specific heat as water? Step 4 Substitute in values and solve.

Learning Check When 8.81 kJ is absorbed by a piece of iron, its temperature rises from 15 ° C to 122 ° C. What is its mass, in grams?

Solution When 8.81 kJ is absorbed by a piece of iron, its temperature rises from 15 ° C to 122 ° C. What is its mass, in grams? Step 1 Given 8.81 kJ SH(iron) = 0.452 J/g ° C 15 ° C to 122 ° C Need mass of iron

Solution When 8.81 kJ is absorbed by a piece of iron, its temperature rises from 15 ° C to 122 ° C. What is its mass, in grams? Step 2 Calculate the temperature change. ΔT = 15 ° C – 122 ° C = 107 ° C Step 3 Write the heat equation.

Calculating Heat Loss When 8.81 kJ is absorbed by a piece of iron, its temperature rises from 15 ° C to 122 ° C. What is its mass, in grams? Step 4 Substitute in values and solve.