Aim: How to measure energy absorbed during a phase change DO NOW: 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature.

Slides:



Advertisements
Similar presentations
Just to review before we start…
Advertisements

Phase Changes Matter can change from one form to another. As this occurs, energy also changes.
Heating/Cooling Curve & Energy Calculations. Which of the following measures the average kinetic energy of a sample? 1.Mass 2.Volume 3.Specific heat 4.Temperature.
Aim: How to measure energy absorbed during a phase change
Calculations in Chapter 10. Molar Enthalpy of Fusion Used when melting or freezing = ___energy ____ mol of substance Can be arranged to find any of the.
Ch. 11 Thermochemistry.
Heating and Cooling Curve Definitions: Specific Heat: Amount of energy required to raise the temperature of 1 gram of a substance by 1⁰ Celsius Enthalpy.
What is the relationship between heat and temperature?
Calorimetry How to use math to describe the movement of heat energy Temperature Change Problems Temperature Change Problems Phase Change Problems Phase.
Energy & Chemical Change
States of Matter Solid Lowest energy/heat Molecules barely moving Definite, uniform shape Example: ice.
Video 5.1 Q=mcΔT. Table I 0 Exothermic reactions release heat and have negative values. 0 Example: When Carbon and Oxygen react they release 393.5kJ of.
Chemistry is about to heat up… Please get out: 1.Last Large Group Notes 2.This Large Group Notes 3.Calculator THERMOCHEMISTRY.
Calculating Heat. Specific Heat Amount of heat energy needed to raise the temp of 1 ml of a substance 1°C For water the specific heat is 4.19 J/g °C,
Matter and Energy When Matter and energy interact changes in matter occur.
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.
Heat: Phase Change. 'change of phase' 'change of state'. The term 'change of phase' means the same thing as the term 'change of state'. o These changes.
Chapters 13 & 17 Phases and Heat. Phases of Matter Chapter 13.
Heat in Changes of State
Part One Heat and Temperature.
Energy.
Calorimetry How to use math to describe the movement of heat energy Temperature Change Problems Temperature Change Problems Phase Change Problems Phase.
THERMOCHEMISTRY: HEAT and CHANGE. When a material is heated (or cooled), it can undergo one of these changes: Its temperature changes OR Its physical.
Water phase changes constant Temperature remains __________
Molar Enthalpy of Vaporization
CALCULATING HEATS OF RXNS o Any phase change requires energy. either energy is absorbed (melting or vaporizing) either energy is absorbed (melting or.
Test #3 Phase Changes. How much heat energy does it take to warm, melt, or boil a substance? ~~ Calorimetry ~~ q = m c  T q = m H f q = m H v q = heat.
Regents Chemistry   Anything that has mass and takes up space  3 states/phases of matter  Solid  Liquid  Gas Lesson 1:What is matter?
2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt Definitions States of Matter Heating.
Aim: How to measure the amount of heat released during a phase change
Topic 4 Transformations and Conservation of Energy.
Phase Changes in Water AIM: How does the Atmosphere store energy?
Calorie (energy) Calculations A calorie is defined as the amount of energy it takes to raise the temperature of one gram of water by one degree Celsius.
October 22  Objective  To represent the changes of energy that occur while a substance is being heated.
Measuring Changes of Heat and Temperature over time. “It was the heat of the moment”
Reaction Energy.
Thermochemical Calculations
Energy Changes & Phase Changes. It takes energy to heat stuff up! For pure substance in single phase, can calculate how much using Q = mC  T For pure.
Energy and Phase Changes. Energy Requirements for State Changes To change the state of matter, energy must be added or removed.
Chapters 13 & 17 Phases and Heat. Phases of Matter Chapter 13.
Phase Changes.  A PHASE CHANGE is a reversible physical change that occurs when a substance changes from one state of matter to another  The temperature.
Energy Changes & Phase Changes Heating & Cooling Curves.
EQ: How can we measure the amount of heat released or absorbed in a chemical reaction? Do Now: What is the difference between potential energy and kinetic.
Calculating Heat During Change of Phase Heat Added (J)
Reaction Energy Specific Heat u The specific heat of any substance is the amount of heat required to raise the temperature of one gram of that substance.
Heating Curves and Energy. Which of the following measures the average kinetic energy of a sample? 1.Mass 2.Volume 3.Specific heat 4.Temperature 5.Heat.
Specific Heat Capacity. Imagine… A hot day in Arizona…in your back yard is a metal barbeque and a glass of water. Would you want to stick your hand in.
Energy in Phase Changes. System vs. Surroundings The system is the part of the universe that interests us, i.e. the reactants and products in a chemical.
CHAPTER 10 Reaction Energy Visual Concepts Heat Chapter 10.
REVIEW 1.Write a formula for the freezing of water. 2.Write a formula for the boiling of water. 3.Write a formula for the condensing of water. 4.Write.
Just What Is It How Can We Define Energy The capacity to do work Or the ability to cause a change to occur.
Measurement of Heat Energy. The amount of heat given off or absorbed in a reaction can be calculated by a) q=mc∆T(Table T) q= heat (in joules or calories)
Thermochemistry Chapter 17. Thermochemistry Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state of.
Unit: ENERGY Topic 1: Types of Energy Energy = The ability to do work or produce heat Unit of energy = the Joule = J Two types: Potential Kinetic Lord.
Unit 4 Thermodynamics. HEATING AND COOLING CURVES.
Types of energy POTENTIAL ENERGY : STORED ENERGY. The energy inside the substance. KINETIC ENERGY : Associated with motion. Average KE = TEMPERATURE.
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.
Phases of Matter, Bonding and Intermolecular Forces
Energy and Physical Changes – Part II
Heating Curve Turk.
Aim: How to measure energy absorbed during a phase change??
Heat In Changes of State of Matter
Thermochemical Calculations
Heating and Cooling Curves
Jeopardy Freezing Melting Heat and Its Meas. Vapor Pressure
Changes of State units: J/g Heat of Vaporization
Warm-up What is the final temperature of a 25.0 g piece of metal if it absorbs 1122 joules of heat and its specific heat capacity is J/g°C? The.
Heating Curves Phase changes & Energy.
October 24 Objectives Describe what happens with PE and KE as phase changes Identify MP and BP from heating curve MP=FP and PB=condensation point Define.
Presentation transcript:

Aim: How to measure energy absorbed during a phase change DO NOW: 1. A g piece of iron absorbs joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron. 2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C? 3. To what temperature will a 50.0 g piece of glass raise if it absorbs 5275 joules of heat and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is 20.0°C.

Energy is absorbed Energy is released

Vocab Potential Energy- stored energy Kinetic Energy- energy having to do with motion Heat of Fusion- the amount of heat needed to change solid to liquid at constant temperature Heat of Vaporization- the amount of heat needed to change liquid to gas at constant temperature

Heat of Fusion amount of heat needed to be absorbed to convert a unit of mass of a substance from a solid to a liquid at its melting point q= mH f Look at Table B: heat of fusion for water is 334 joules per gram. Example: How many joules are required to melt 255 g of ice at 0 o C?

Heat of Vaporization amount of heat needed to be absorbed to convert a unit mass of a substance from its liquid phase to gas phase. q = H v m Look at Table B: heat of vaporization for water is 2260 joules per gram. Example: How many joules of energy are required to vaporize 423 g of water at 100 o C and 1 atm?

Practice 1.What is the heat of solidification for 3.4 g of water? 2. How much energy is released to the environment by 50.0 grams of condensing water vapor? 3. Is melting endothermic or exothermic? Explain.

Practice 4. Calculate the amount of heat needed to melt 35.0 g of ice at 0 ºC. Express your answer in kilojoules. 5. How many joules must be added to 10.0g of water to raise its temperature from 10 C to 15 C.

q=mH f q=mH v

Heating Curve 1.Temperature of the ice (solid) is increasing; increase in temperature means an increase in kinetic energy. 2.At 0 o C the ice begins to melt. During melting, the temperature stays the same; there is no change in kinetic energy. There is a change in potential energy; potential energy is increasing. 3.The temperature of the water now rises from 0 o C to 100 o C.

Heating Curve 4. At 100 o C, the water boils (changes to gas). When the water boils, the temperature stays the same; no change in kinetic energy. There is a change in potential energy; potential energy increases. 5. After all the water boils, the temperature of the gas rises.