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Transcript of Thermodynamics Day 1. Section 1 Notes: Temperature Scales and Conversions Intro Question 1. How...
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Thermodynamics
Day 1
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Section 1 Notes: Temperature Scales and Conversions
Intro Question
1. How does a thermometer determine temperature?
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Thermodynamics (Unit 1 spring)
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• Thermodynamics- Physics that deals with heat and its conversion into other forms of energy.
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Video Clip: The Thermometer
• 1:36
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Video Clip: Fahrenheit and Celsius Scales• 5:14
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Temperature Variables
• TK= Temperature Kelvin
• TC= Temperature Celsius
• TF= Temperature Fahrenheit
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Video: Absolute Zero
• 1:49
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• Absolute Zero= 0 Kelvin, a temperature where no motion would occur. There is no kinetic energy in the molecules.
• 0 Kelvin= -273.15 ºCelsius
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Conversion Scale
( )
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Example 1
• A healthy person has an oral temperature of 98.6 ºF. What would this reading be on the Celsius scale?
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Example 1
• A healthy person has an oral temperature of 98.6 ºF. What would this reading be on the Celsius scale?
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Example 2
• A time and temperature sign on a bank indicates the outdoor temperature is -20.0 ºC. What is the corresponding temperature on the Fahrenheit scale?
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Example 2
• A time and temperature sign on a blank indicates the outdoor temperature is -20.0 ºC. What is the corresponding temperature on the Fahrenheit scale?
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The Kelvin Temperature Scale• Has scientific significance
due to its absolute zero point.
• Has equal divisions as the Celsius scale
• Not written in degrees• 0º C is 273.15 K• Therefore the conversion is:
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• CP: – Finish Worksheet Problems 1-4
• Honors: – Finish Worksheet Problems 1-4
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Day 2
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Intro
1. Convert 50º F into ºC and Kelvin
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Intro
1. Convert 50º F into ºC and Kelvin
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Intro
1. Convert 50º F into ºC and Kelvin
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Video: Voyage up the Celsius Scale• 11:09
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Section 2 Notes:Kinetic Energy and Temperature
• Kinetic energy (KE)- Energy of movement
• Temperature- A measure proportional to the average kinetic energy of a substance.
– higher temperature = higher kinetic energy– The more kinetic energy the quicker the molecules are
moving around
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Click on the diagram to be taken to the page
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• Draw a picture representing molecular motion of three identical molecules at these two temperatures
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• Draw a picture representing molecular motion of three identical molecules at these two temperatures
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Section 3 Notes: Internal Energy vs. Heat
• Internal energy (U)- Sum of the molecular energy– kinetic energy, potential energy, and all other energies
in the molecules of a substance. – Unit: Joule
• Heat (Q) is energy in transit– energy flows from a hot to a cold substance.– Unit: Joule
• An object never has “heat” or “work” only internal energy (heat is transferred and work is done)
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Heat is energy in transit
• Heat lost by one object equals heat gained by another
• Heat lost = Heat gained• -QA = QB
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Heat transfers from hot to cold
(a) Holding a hot cup
(b) Holding a cold glass (heat leaving your hand feels cold)
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• The coffee looses 468J of heat. How much heat does Bob gain? (assuming no heat was lost to the surroundings)
• The same: Bob gained 468 J of heat
Example 3
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– Direction: From high temperature to low temperature
– Rate of transfer depends on temperature difference: The greater temperature difference the greater the energy transfer
Twater =
20º C
Tcan =
15º C
Twater =
35º C
Tcan =
5º C
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Example 4
Where would the greater energy transfer take place and which way would the energy transfer?
A. Ice = 0 ºC Juice = 20 ºC
B. Ice = 0 ºC Juice = 25 ºC
B. has a bigger temperature difference and therefore greater energy transfer. Energy transfers from hot to cold: Juice to Ice
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What happens when the temperature inside and out are equal?
Twater =
11º C
Tcan =
11º C
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• Heat is transferred until there is thermal equilibrium
• Thermal Equilibrium- When temperatures are equal and there is an even exchange of heat
Twater =
11º C
Tcan =
11º C
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Section 4 Notes: Heat Transfer
• Types of Heat Transfer:
– Conduction– Convection– Radiation
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• Conduction- Caused by vibrating molecules transferring their energy to nearby molecules. Not an actual flow of molecules.
heat transfer
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• Thermal conductors- rapidly transfer energy as heat
• Thermal insulators- slowly transfer energy as heat
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Challenge
• Put the following in order of most thermally conductive to least.
Copper, Wood, Air, Water, Concrete
12345
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1. Copper
2 Concrete
3. Water
4. Wood
5. Air
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• Convection- process in which heat is carried from place to place by the bulk movement of a fluid (gas or liquid).
• Examples
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• Radiation (electromagnetic radiation) – Reduce internal energy by giving off electromagnetic radiation of particular wavelengths or heated by an absorption of wavelengths.
• Ex. The UV radiation from the
sun making something hot. Absorption
depends on the material.
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Draw your own pictures in the table that represent these three types of heat transfer.
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Draw your own pictures in the table that represent these three types of heat transfer.
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CW
• Finish questions 5 and 6 on the worksheet
Heat Video if time allows
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Day 3
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Intro
• Intro question/activity:– Draw these two tables in your intro section. In (a) represent the
motion of three identical molecules at these two temperatures. In (b) draw a picture representing these three types of heat transfer. Try not to look at your notes until you are done.
(a) (b)
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Intro
• Draw a picture representing molecular motion of three identical molecules at these two temperatures
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Intro
Draw your own pictures in the table that represent these three types of heat transfer.
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Section 5: Laws of Thermodynamics
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A System
• System- A collection of objects upon which attention is being focused on.
• This system includes the flask, water and steam, balloon, and flame.
• Surroundings- everything else
in the environment
The system and surrounding are
separated by walls of some kind.
System
Surroundings
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Walls between a system and the outside
• Adiabatic walls- perfectly insulating walls. No heat flow between system and surroundings.
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In a system: How can you measure the quantity of heat entering or leaving?
Q = Δ U or Q = Uf – U0
• Q: The quantity of heat that enters or leaves a system• U0: Initial internal energy in system• Uf: Final internal energy in system
• If Q is positive then energy entered the system• If Q is negative then energy left the system
• This is directly related to temperature. – If the system gets colder then heat left– If the system gets warmer then heat entered
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Example 5
• The internal energy of the substance is 50 J before
• The internal energy of the substance is 145 J after
a) How much heat was transferred in this system? b) Did it enter or leave?
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• First Law of Thermodynamics:
– Conservation of energy applied to thermal systems.
– Energy can neither be created nor destroyed. It can only change forms
– Stated in an equation
ΔU = Q + W
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First Law of Thermodynamics: Conservation of Energy
ΔU = Q + W
– Internal Energy (U) • (positive if internal energy is gained)
– Heat (Q) • (positive if heat is transferred in)
– Work (W)
• (positive if work is done on the system)
– The unit for all of these is the Joule (J)
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Example 6 & 7
6. A system gains 1500 J of heat from its surroundings, and 2200 J of work is done by the system on the surroundings. What is the change in internal energy?
7. A system gains 1500 of heat, but 2200 J of work is done on the system by the surroundings. What is the change in internal energy?
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6. A system gains 1500 J of heat from its surroundings, and 2200 J of work is done by the system on the surroundings. What is the change in internal energy?
7. A system gains 1500 of heat, but 2200 J of work is done on the system by the surroundings. What is the change in internal energy?
1500 - 2200
1500 + 2200
Example 6 & 7
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Now how can you tell if work is done by or on a system?
Is work done on or by the system ?a) nail/wood system b) Bunsen burner,
flask, balloon system
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• Work is done by the man causing frictional forces between the nail and the wood fiber.
• Work increases the internal energy of the wood and nail.
Work done on a system:Work to Internal Energy
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Work done by a system:Internal Energy to Work
• The balloon expands doing work on its surroundings
• The expanding balloon pushes the air away
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Work done on or by a gas
• Volume must change or no work is done.
• On a gas- Volume decreases (work must be done to force molecules into a smaller area)
• By a gas- Volume increases (the pressure of the gas causes the volume to increase)
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Section 5 Notes
4 Common Thermal Processes• Isobaric Process • Isochoric process (isovolumetric)• Isothermal process • Adiabatic process
• Each will have their own assumptions
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4 Thermal Processes
• Isobaric Process – occurs at constant pressure
• ΔP = 0
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4 Thermal Processes
• Isochoric process (Isovolumetric) – one that occurs at constant volume.
• ΔV = 0 and therefore W = 0
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Thermal Processes
• Isothermal process – one that occurs at constant temperature
• T (temperature) directly relates to U (internal energy)
• ΔU = 0
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Thermal Processes
• Adiabatic process – on that occurs with no transfer of heat
• ΔQ = 0
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Look for these terms in questions since they assume givens
• Isobaric Process ΔP = 0• Isochoric process ΔW = 0• Isothermal process ΔU = 0• Adiabatic process ΔQ = 0
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Example 8
• How much heat has entered or left the system when 500J of work has been done on the system in an isothermal process?
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Example 8
• How much heat has entered or left the system when 500J of work has been done on the system in an isothermal process?
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Example 9
• How much work is done on or by the system when internal energy increases by 55J in n adiabatic process?
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Example 9
• How much work is done on or by the system when internal energy increases by 55J in n adiabatic process?
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CW/HW
• Do the first law of thermodynamics questions 7-10 on the worksheet
• Define the 16 words on the worksheet
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Day 4
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Intro
1. What does an adiabatic process tell you?
2. What does an isovolumetric process tell you?
3. What does an isothermal process tell you
4. How much work is done on or by the system when internal energy decreases by 45J in an adiabatic process?
5. What is the change in internal energy if 650 J of work is done and 50J of heat is transferred in?
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Section 6: Three Laws of Thermodynamics
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First Law of Thermodynamics
1. Energy can neither be created nor destroyed
• Energy Conservation: Conservation of energy applied to thermal systems.
• . It can only change forms
• When heat is added to a system, it transforms to an equal amount of some other form of energy.
• Equation:• ΔU = Q + W (work is done on a system)
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Second Law of Thermodynamics2. Entropy in a system increases over time. Entropy- Measure of randomness or disorder in a system
This occurs even when a system is left untouched.Other parts of the second law of thermodynamic
• Heat goes from hot to cold.• No cyclic process is 100% efficient • it can’t convert heat entirely into work • Some energy will always be transferred out to
surroundings as heat.
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Third Law of Thermodynamics
3. absolute zero cannot be reached
• As a system approaches absolute zero, all processes cease and the entropy of the system approaches a minimum value.
• A theoretical impossibility– If it occurred everything would stop and there
would be no more entropy
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Section 7: Transformation of energy in a heat engine
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The Heat Engine– a device that used a difference in temperature of two
substances to do mechanical work – It transferring energy from a high-temperature
substance (the boiler) to a lower temperature substance
– For each complete cycle: Wnet = Qh - Qc
What the variables stand for here:
Qh = Heat from high temperature substance
Qc = Heat to low temperature substance
W or work equals the difference of Qh and Qc
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The Heat EngineHow it works: main points
There will be an area of high temperature (boiler) and an area of low temperature
• Heat wants to go from a high temperature to a low temperature.
• Work is done by capturing energy in the transfer and using it to do work
• The work done by the engine equals the difference in heat transferred from the hot to cold substance.
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The Heat Engine–For each complete cycle: Work =
Energy transferred as heat from the high temperature substance to the colder temperature substance
What the variables stand for here:
Qh = Heat from high temperature substance
Qc = Heat to low temperature substance
W or work equals the difference of Qh and Qc
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Example 10
• A heat engine is working at 50% efficiency. How much work is done between a 670J and 200J reservoir?
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Example 10
• A heat engine is working at 50% efficiency. How much work is done between a 670J and 200J reservoir?
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Example 11: (just added and not on your worksheet)Do this question on free space below example 10
A heat engine has a 5000 J reservoir and a 2000J reservoir. If the engine can does 2100J of work, how efficient is it?
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•
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•
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•
Question 1:
Which law of thermodynamics relates to the 5000J and 2000J
reservoir and the direction of heat transfer and not being 100% efficient?
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•
Question 1:
Which law of thermodynamics relates to the 5000J and 2000J
reservoir and the direction of heat transfer and not being 100% efficient?
Second Law of thermodynamics (Entropy)
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Nuclear Physics
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Intro:
1. What atom is this?
2. Where do you find protons?
3. Where do you find neurons?
4. Where do you find electrons?
5. How many protons does it have?
6. How many neutrons?
7. Is it a neutral atom, and how do you know?
ALL CLASSES MEET IN COMPUTER LAB 1.618 TOMORROW
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The Atom
In the nucleus (nucleons)
Proton- (+) charged particle
Neutron- no charge
Outside the nucleus
Electron- (-) charged particle
has almost no mass
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Nucleons
• Are particles occupying the nucleus• Consist of + charged protons and neutral
neutrons• Have almost 2000 times the mass of
electrons
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• Where can you find the number of protons? • It’s the atomic number (found on the periodic
table)
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Nuclear Notation
Atomic number = no. of protons
Atomic mass = protons + neutrons
Atomic number is the same as the number of electrons in an uncharged atom
5
B10.811
Atomic Number
Atomic Mass
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1a. How many protons?
1b. How many neutrons?
1c. How many nucleons?
You may see atomic number written many ways. The smaller number is the atomic number and the larger is the atomic mass
Question 1
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• has 13 protons and 14 neutrons for a total of 27 nucleons
• has 13 protons and 15 neutrons for a total of 28 nucleons
• The identity of an element depends on the number of protons
2813
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Isotopes:
• Atoms of the same element with different numbers of neutrons (different masses)
Most common stable isotope of carbon
Unstable radioactive isotope of carbon
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Question 2
• List the four fundamental forces from strongest to weakest
1.
2.
3.
4.
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Review of Fundamental forces
Strongest to weakest1. Strong Nuclear Force
2. Electromagnetic Force
3. Weak Nuclear Force
4. Gravity
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Forces Acting on Nucleons:
Forces of attraction between nucleons
Strong forces– Are independent of the charge of the nucleon– Are short range (exist only between closest
neighbors)
Electrical force (electrostatic)– Force of repulsions between positively
charged protons– Are long range
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When are nuclei unstable? (naturally radioactive)
a. Large nuclei (Z > 82) – electrical forces of repulsion are greater than strong forces of attraction
b. Wrong neutron : proton ratio
stable nucleus no. of protons no. of neutrons
6 6
13 14
26 30
56 81
82 125
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When are nuclei unstable?
Bigger atoms require more neutrons per proton to keep the atom stable
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A radioactive isotope:
• Has an unstable nucleus
• Spontaneously emits a particle and decays into another element (to become more stable)
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Transmutation
• Changing into another element through radioactive decay
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• I worked with my husband and discovered radium, a radioactive material
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Marie and Pierre Curie
• First to discover that compounds containing uranium emitted penetrating rays.
• Discovered radioactive polonium and radium
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Types of Radioactive Emission
Symbol Composition Stopped By
Alpha 2p + 2n (helium)
Paper
Beta 1e (electron)
Aluminum
Gamma γ Energy only
Lead
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Use a periodic table for decay equations
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Alpha Decay
• Radiation through the loss of 2p + 2n or (helium)
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Beta Decay
• Radiation where a neutron splits, giving off an electron and becoming a proton in the new element
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Gamma Decay
• A change energy state gives off a gamma particle or photon
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Question 3a
Balance the nuclear equation after alpha decay
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Question 3a
Balance the nuclear equation after alpha decay
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Question 3b
Balance the nuclear equation after beta decay
Remember in beta decay a neutron changes into a proton by giving off an electron
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Question 3b
Balance the nuclear equation after beta decay
Remember in beta decay a neutron changes into a proton by giving off an electron
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Extra Question
• Which radioactive isotope completes this nuclear decay equation
6
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Extra Problem
• Finish off the equation
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Half Life and Half Life Calculations
• Half Life- time it takes for half of the radioactive sample to decay.– Ranges from a fraction of a
second to billions of years
• Decay constant- Probability per time that a nucleus would decay
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CW/HW
• Do Page 1 of the worksheet: Nuclear and Thermodynamics Extra Practice
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Section 2 Intro
1. Rewrite and balance the equation above
2. What kind of decay is shown above?
3. What is the particle given off during alpha decay composed of?
4. What is the particle given off during beta decay composed of?
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Section 2: Nuclear Physics Math
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Half Life Calculations
Draw and finish off the table in your notes
# of Half Lives Fraction Remaining
Fraction Decayed
How much of 100g sample left
How much of 100g sample decayed
0 1.0 0 100g 0
1
2
3
4
5
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Half Life and Half Life Calculations
y= fraction of radioactive material left
n= number of half lives
T1/2 = half life time
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Example A
• How much of the original radioactive material is left after 15 half-lives?
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Example A
• How much of the original radioactive material is left after 15 half-lives?
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Not every radioactive isotope is created equal
Parent Decays into: Half life (years)
Carbon-14 Nitrogen-14 5,730
Aluminum-26 Magnesium-26 740,000
Iodine-129 Xenon-129 17 million
Uranium-235 Lead-207 704 million
Potassium-40 Argon-40 1.3 billion
Rubidium-87 Strontium-87 49 billion
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Example B
• We start with 400g of a sample, how many grams would remain after 3 half lives?
#1 figure out the fraction remaining (y)
#2 multiply the fraction remaining by the mass of the original sample (y) x (mo)
mo = initial mass of radioactive material
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Example B
•
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Example C
• A radioactive sample has a mass of 56 mg and a half life of 30 minutes. How much of the sample remains after 60 minutes have passed?
• Step#1 find number of half lives (n)• Step#2 find what fraction remains (y)• Step#3 if an initial sample was given multiply
fraction remaining (y) x (the initial sample mass)
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Example C
• A radioactive sample has a mass of 56 mg and a half life of 30 minutes. How much of the sample remains after 60 minutes have passed?
• Step#1 find number of half lives (n)
Rearranges to
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Example C
• A radioactive sample has a mass of 56 mg and a half life of 30 minutes. How much of the sample remains after 60 minutes have passed?
• Step#1 find number of half lives (n) = 2• Step#2 find what fraction remains (y)
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Example C• A radioactive sample has a mass of 56 mg
and a half life of 30 minutes. How much of the sample remains after 60 minutes have passed?
• Step#1 find number of half lives (n) = 2• Step#2 find what fraction remains (y) = 0.25
• Step#3 if an initial sample was given multiply fraction remaining (y) x (the initial sample mass)
• 56 x 0.25 = 14 grams
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Example D
• An unknown radioactive material has a half life of 4000 years. How much of the sample will remain after 20,000 years?
Rearranges to
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Example D
• An unknown radioactive material has a half life of 4000 years. How much of the sample will remain after 20,000 years?
Rearranges to
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Example E•
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Example E•
(n) Number of half lives
original 1 2 3 4 5
Quantity remaining 32g 16g 8g 4g 2g 1g
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Example E•
(n) Number of half lives
original 1 2 3 4 5
Quantity remaining 32g 16g 8g 4g 2g 1g
2. What is the T1/2
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Example E•
(n) Number of half lives
original 1 2 3 4 5
Quantity remaining 32g 16g 8g 4g 2g 1g
2. What is the T1/2 = 18/5
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Useful applications of radioactivity• Can be detected and therefore small
amounts can be used as tracers for medical diagnosis
• Larger amounts can be used as treatments for certain types of cancers (cancer cells are killed before healthy cells)
• Can be used to determine the age of rocks and fossils
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Show what you know
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Types of Nuclear Reactions
Natural transmutation – Uranium spontaneously decays
Artificial transmutation – bombardment of a stable isotope to force it to decay
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Question 4
• Balance the reaction after the following artificial transmutation.
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Types of Nuclear Reactions
Artificial transmutation • First done by Earnest Rutherford
• When the bullets are positively charged, they are repelled by the nucleus they are bombarding. To overcome the repulsions, they must be accelerated to very high speeds by particle accelerators.
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Nuclear Fission
• Nuclear fission - Heavy nuclei are bombarded with neutrons and split.
plus a tremendous amount of energy
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Nuclear fission
• Mass of particles produced is slightly less than the mass of the reactants. This mass is converted into energy. (E=mc2)
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Nuclear fission is a chain reaction. Neutrons are needed to start and released as a product which can start more reactions.
Critical mass: minimum mass of fissionable material required for a chain reaction.
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Problems with Fission• Nuclear fission produces radioactive waste that has
a large half life.
U-235 Uranium 235
– Half life of U-235 is 713 million years
• We cannot get rid of this dangerous product so we store it away from anything it can harm.– We deeply bury
• Meltdown if cooling system fails the reactor can overheat and melt releasing radioactive materials
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• Nuclear fusion – combination of small nuclei into larger with release of energy.
• Mass of particles produced is much less than the mass of the reactants.
• This mass is converted into energy. (E=mc2)• Can release up to 10 times that of fission• Occurs naturally in our sun and other stars• Does not give off radioactive waste
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Problems with Fusion
• Fusion requires high temperatures like those in the stars.
• We cannot sustain these temperatures without vaporizing the container of the fusion reaction.
• Today many are looking into ways of making fusion work under sustainable conditions