Thermodynamics & Phase Change. Heat can only do one thing at a time: either change the temperature OR change the state!

Slides:

Advertisements

Similar presentations

 State of Balance For the phase changes: As many molecules evaporating as there are condensing.

Advertisements

The rope ladder of a boat hangs over the side of the boat and just touches the water. The ladder rungs are 8 inches apart. How many rungs will be under.

Energy and Phases. Potential Energy - stored energy (stored in bonds, height) Kinetic Energy - energy of motion, associated with heat.

L 19 - Thermodynamics [4] Change of phase ice  water  steam

Brief walk-through of temperature, heat, and energy transfer

Heat Chapter 9 &10. Kinetic-molecular Theory Matter is made up of many tiny particles that are always in motion In a hot body the particles move faster.

Thermodynamics Notes Section: 10.4.

Heat, Temperature, Heat Transfer, Thermal Expansion & Thermodynamics.

Heat, Temperature, Heat Transfer & Thermodynamics

Chapter 11 Energy in Thermal Processes. Energy Transfer When two objects of different temperatures are placed in thermal contact, the temperature of the.

Important Terms & Notes Conceptual Physics Mar. 12, 2014.

1 L 19 - Thermodynamics [4] Change of phase ice  water  steam The Laws of Thermodynamics –The 1 st Law –The 2 nd Law –Applications Heat engines Refrigerators.

Chapter 14 Heat and Temperature: Temperature Energy Transfer Using Heat.

Thermal Energy Milbank High School. Sec Temperature and Thermal Energy Objectives –Describe the nature of thermal energy –Define temperature and.

Thermodynamics is a Study of heat. A major topic of in this field Is the Kinetic-Molecular Theory.

Thermodynamics.

Pre-AP Physics Unit 6: Thermodynamics. “Thermodynamics”  Is derived from Greek meaning “movement of heat.”

Part One Heat and Temperature.

A 50.0 g ball is dropped from an altitude of 2.0 km. Calculate: U i, K max, & W done through the fall.

Physics Unit 6: Thermodynamics

Unit 12: Thermodynamics Think of a steam engine:.

Energy and energy transformations. First Law of Thermodynamics  Energy is never created nor destroyed Energy can change forms, but the quantity is always.

Thermodynamics is a Study of heat. A major topic of in this field Is the Kinetic-Molecular Theory.

Change of State and Laws of Thermodynamics

Heat, Work, and Internal Energy Thermodynamic Processes.

VII. The second low of Thermodynamics

Chapter 12 Thermal Energy Glencoe 2005 Honors Physics Bloom High School.

Chapter Thermal Energy 12.

Heat, Temperature, Heat Transfer, Thermal Expansion & Thermodynamics.

Laws of Thermodynamics Thermal Physics, Lecture 4.

Important Terms & Notes Conceptual Physics Mar. 17, 2014.

NS 3310 – Physical Science Studies

Conservation of Energy

Kinetic-Molecular Theory States that matter is made up of many tiny particles that are always in motion.

Thermodynamics. Thermodynamics – The study of heat transformation. Temperature – A measure of the average kinetic energy of the particles in an object.average.

Thermodynamics & Phase Change. Heat can only do one thing at a time: either change the temperature OR change the state!

Energy and Phases.  Potential Energy - stored energy (stored in bonds, height)  Kinetic Energy - energy of motion, associated with heat.

C h a p t e r 1 2 T h e r m a l E n e r g y Section 12.1 Temperature and Thermal Energy Section 12.2 Change of State & Laws of Thermodynamics.

Heating Curves. Energy and Phase Change When adding heat to a solid, energy added increases the temperature and entropy until the melting point is reached.

Chapter 17 Energy in Thermal Processes: First Law of Thermodynamics.

Temperature: Is that property of a system which equals that of another system when the two system are in thermal equilibrium. Or Is the physical property.

Matter and Energy Pg  All physical and chemical changes involve a change in energy  Energy goes in or energy comes out.  If energy goes in.

Chapter 12: Thermal Energy What’s hot and what’s not…

Thermochemistry. Thermochemistry is the study of heat changes that occur during chemical reactions. Heat (q) - energy that is transferred from one object.

Reaction Energy.

Energy Solving Quantitative Energy Problems

Chapter 5 Thermal Energy

Thermal Energy  Temperature  Thermal Energy  Heat Transfer.

Thermodynamics Ch 21 to 24 Regelation When water is frozen and pressure is applied to a certain area, that area will melt – then immediately refreeze.

10-3: Changes in Temperature and Phase Objectives: Perform calculations with specific heat capacity. Perform calculations involving latent heat. Interpret.

Energy for Heat Transfer. 1 st Law of Thermodynamics Whenever heat flows into or out of a system, the gain or loss of thermal energy equals the amount.

Conservation of Energy. Law of Conservation of Energy (p222) The law of conservation of energy states that energy cannot be created nor destroyed, but.

Chapter 12 Thermal Energy.

CH. 12 Thermal Energy Sec. 12.1: Temperature & Thermal Energy.

Change of States and Laws of Thermodynamics Chapter 12.2 pg

Chapter 3.1 Laws of Thermodynamics. Systems  A system is a set of interconnected parts  An open system is one that exchanges both matter and energy.

Calculating Heat During Change of Phase Heat Added (J)

Thermal Energy Chapter 12 Physics Principles and Problems Zitzewitz, Elliot, Haase, Harper, Herzog, Nelson, Nelson, Schuler and Zorn McGraw Hill, 2005.

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.

Objectives  Define heats of fusion and vaporization.  State the first and second laws of thermodynamics.  Distinguish between heat and work.  Define.

Thermal Energy & Heat 1.Temperature – The measure of the average kinetic energy of the particles that make up a substance. 2.Temperature Scales – Fahrenheit,

Chapter 16 Thermal Energy & Heat.  Objectives:  1. Explain how heat and work transfer energy  2. Relate thermal energy to the motion of particles that.

Heat, Temperature, Heat Transfer, Thermal Expansion & Thermodynamics.

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.

THERMAL ENERGY.

Heating and Cooling Curves

Heat, Temperature, Heat Transfer, Thermal Expansion & Thermodynamics

Chapter 19 Heat and the First Law of Thermodynamics

Heat, Temperature, & Thermodynamics

Heat, Temperature, Heat Transfer, Thermal Expansion & Thermodynamics

Presentation transcript:

Thermodynamics & Phase Change

Heat can only do one thing at a time: either change the temperature OR change the state!

Changes of state – seen in phase change diagram temperature heat added

Diagonal regions: where thermal energy is added and particles increase in motion (temperature changes) Flat regions: where changes in state occur. All added thermal energy goes to overcome the forces holding the particles together.

Heat of fusion – The amount of energy required to melt one kilogram of a substance Heat of vaporization – the amount of energy required to vaporize one kilogram of a substance

Heat of Fusion & Vaporization for Water Heat of fusion for water: H f = 3.34x10 5 J/kg positive when melting, negative when freezing Heat of vaporization for water: H v = 2.26x10 6 J/kg positive when evaporating, negative when condensing

Heat required to melt: Q = mH f *use for melting & freezing! Heat required to vaporize: Q = mH v *use for evaporating & condensing!

Specific Heat Values C ice = 2060 J/kg·˚C C water = 4180 J/kg·˚C C steam = 2020 J/kg·˚C Use these values for temps in Celsius or Kelvin!

Example #1 You are asked to melt kg of ice at its melting point and warm the resulting water to 20.0 ºC. How much heat is needed?

Calculate heat needed to melt the ice. Q 1 = mH f Calculate heat needed to raise water temperature. Q 2 = mCΔT Add all heats together to get the total heat needed. Q = Q 1 + Q 2 Example #1 Strategy:

Example #1 Solution: Q 1 = J Q 2 = 8360 J Q = 41,760 J

Example #2 A 40.0-g sample of chloroform is condensed from a vapor at 61.6 ºC. It liberates 9,870 J of heat. What is the heat of vaporization of chloroform?

Example #2 Solution: Q = mH v = (.040)(H v ) H v = -246,750 J/kg (negative because it’s cooling)

Law of Conservation of Energy Energy cannot be destroyed or created only transferred.

1 st Law of Thermodynamics The total increase in the thermal energy of a system is the sum of the heat added to it and the work done on it. Heat engines are devices which convert thermal energy to mechanical energy continuously along with some waste heat.

2 nd Law of Thermodynamics Entropy of the universe is always maintained or increased. All things will become more and more disordered unless some action is taken.

Entropy is a measure of the disorder in a system. Entropy increases when heat is added and decreases when heat is removed. 2 nd Law of Thermodynamics

Thermal Engine efficiency Called Carnot efficiency, or the ideal efficiency of a heat engine (T hot -T cold )/T hot = Ideal efficiency Temperatures must be in Kelvin. Result is a percentage.