calories

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Where does the energy we use come from?

• Electricity
• Biomass Energy - energy from plants
• Geothermal Energy
• Fossil Fuels - Coal, Oil and Natural Gas
• Hydro Power and Ocean Energy
• Nuclear Energy
• Solar Energy
• Wind Energy
• Transportation Energy

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Source U.S. Energy Information Administration,
Office of Coal, Nuclear, Electric and Alternate
Fuels 
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Courtesy of World Resources Institute, 10 G
Street, NE (Suite 800), Washington, DC 20002
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Courtesy of Uranium Information Center Ltd
Energy for the World - Why Uranium?
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http//www.eia.doe.gov/oiaf/ieo/highlights.html
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http//www.eia.doe.gov/oiaf/ieo/highlights.html
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Courtesy of Economic Energy Report by Michael
Hodges
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PENNSYLVANIA FACTS

• Pennsylvania ranks second in the nation in
  nuclear power generating capacity
• 5 operating power plants that provide 1/3 of the
  electricity needs of the state
• PA is a major coal producing state, selling ½ of
  its coal output to other states
• PA is the leading petroleum refining state in the
  Northeast
• PAs electricity production exceeds state demands
• PA is among the largest users of municipal solid
  waste and landfill gas for electricity generation
• PA produces substantial hydroelectric power
• In December 2004, PA adopted an alternative
  energy portfolio standard that requires
  electricity companies and generators to supply
  18.5 of PAs electricity from alternative energy
  sources by 2020.

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PA's energy producers
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Activity

• With your assigned group members discuss
  solutions to the
• following problem. Come to agreement as a group
  on a
• solution, and choose one member that will present
  your
• solution at the end of class.
• Problem What can be done to meet the
• United States ever-growing energy demands while
• improving the quality of life of todays society
• without sacrificing the quality of life of future
  
• generations?

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Law of Conservation of EnergyEnergy cannot be
created nor destroyed!
Type of Energy Examples
Kinetic Sound, Wind, Spinning Wheel
Potential Ball held above ground, water before a dam
Radiant Light, Microwaves, X-rays, Gamma waves
Electrical Electricity, static cling, lightning
Magnetic Magnets, compasses
Mechanical Pistons in a car engine
Thermal Heat
Nuclear Nuclear fission, nuclear fusion, heavy water
Chemical Gasoline, oil, batteries, food
Spring Stretched rubber band, bungee cord, spring scale
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Law of Conservation of EnergyEnergy cannot be
created nor destroyed!
or from one kind of energy into another kind.
Any situation where energy is transferred from
one object to another
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Rube Goldberg Machine
Draw your final sketch today. Label all 10 forms
of energy associated with your machine.
Webster's Dictionary definition of "rube
goldberg Accomplishing by extremely complex,
roundabout means what seemingly could be done
simply.
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Rube Goldberg Machine

• Objective Make a drawing of a Rube Goldberg
  device of your own creation which includes
  examples of each of the 10 basic types of energy
  and 10 different energy changes.  
• 10 energies - these should be clearly labeled
  and numbered in blue next to where the energy
  occurs in the drawing.
• 10 different energy changes - arrows should be
  drawn connecting each energy in the drawing to
  the next in red to show how one type of energy is
  changing into another.

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Calorie

• Always refers to the energy in food
• A measure of how much potential energy that food
  possesses
• 1 Calorie 1 kilocalorie 1000 calories
• Body burns calories through metabolic processes
• Enzymes break carbohydrates into glucose and
  other sugars, fats into glycerol and fatty acids
  and proteins into amino acids

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Caloric Breakdown

• 1 gram carbohydrates 4 Calories
• 1 gram protein 4 Calories
• 1 gram fat 9 Calories

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Underweight lt5, Healthy 5-85, Risk of
Overweight 85-95, Overweight gt95
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The Bodys Caloric Needs

• 2,000 Calories is an average bodys need
• Height, weight, gender, age and activity level
  all affect a persons caloric needs
• To calculate your bodys needs add together
• basal metabolic rate
• physical activity
• thermic effect of food

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BMR--Basal Metabolic Rate

• Accounts for about 60 to 70 percent of calories
  burned in a day
• Includes the energy required to keep the heart
  beating, the lungs breathing, the kidneys
  functioning and the body temperature stabilized
• Adult male 66 (6.3 x body weight in lbs.)
  (12.9 x height in inches) - (6.8 x age in years)
• Adult female 655 (4.3 x weight in lbs.) (4.7
  x height in inches) - (4.7 x age in years)
• Ms. Wacks BMR 1366.4

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Physical Activity
Sedentary Activities Energy Costs in
Cals/Hour Lying down or sleeping - 90Sitting
quietly - 84Sitting and writing, card playing,
etc. - 114 Moderate Activities (150-350 cal/hr)
Bicycling (5 mph) - 174 Light
housework, cleaning, etc - 246Bicycling (6 mph)
- 240 Swimming (crawl, 20 yards/min)
- 288Dancing (Ballroom) - 210
Gardening - 323Golf (twosome, carrying clubs) -
324 Walking (2 mph) - 198 to 240
Walking (3 mph) - 320 Walking (4
1/2 mph) - 440
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Thermic Effect of Food

• The amount of energy your body uses to digest the
  food you eat
• Multiply the number of calories you eat in a day
  by 10 (0.10)

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Food Serving Size CaloriesAmerican Cheese 1
slice 70Apple 1 medium 80Apple Juice 8
fluid ounces 120Bacon 2 slices 80Bologna 1
ounce 90Caesar Salad 10 oz. w/
dressing 520Carrot, fresh 1 medium 35Cheesecak
e, Plain 1/4 of 19 oz cake 330Cola 8
oz 100French Fries 10 strips 160Frozen
Waffles 2 waffles 220Hamburger 4 oz.
Patty 445Hamburger roll 1 roll 130Macaroni
and Cheese 7.5 ounces 260Milk 8 ounces 160
Pizza, Cheese 1 slice 290Potato Chips 1
ounce 150 Pretzels 1 ounce 110
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Effects of Calorie Intake
Use the handouts on your table to determine the
of calories you eat in an average day (estimate
it). Then use the calculations from yesterday
and the information below to determine whether
you should be losing, gaining or maintaining
weight. Write your answers on your handout from
yesterday.
ATB

• An accumulation of 3500 extra Calories is stored
  by your body as 1 pound of fat
• Lose 1 pound of fat when you burn 3500 more
  calories than you eat
• Burn what you eat to maintain your weight
• Body burns an increased of calories for 2 hours
  after exercise

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What happens when you dont get the Calories you
need?

• Body initially responds with weight loss by
  breaking down fat
• After a few weeks body senses starvation and your
  metabolism will decrease so less overall energy
  is needed
• Body will look for other sources of fuel will
  begin breaking down muscle resulting in loss of
  lean muscle mass (if already underweight can
  result in loss of tissue surrounding internal
  organs, including the heart).
• Symptoms Fatigue, diarrhea, inability to stay
  warm, irritability, weakened immune system,

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calories

• A unit of energy
• The quantity of heat needed to raise the
  temperature of 1 g of pure water 1C

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Calorie

• Always refers to the energy in food
• A measure of how much potential energy that food
  possesses
• 1 Calorie 1 kilocalorie 1000 calories
• Body burns calories through metabolic processes
• Enzymes break carbohydrates into glucose and
  other sugars, fats into glycerol and fatty acids
  and proteins into amino acids

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Joule

• The SI unit of energy
• the symbol for Joule is J
• 1 J 0.2390 cal
• 4.184 J 1 cal

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Energy Conversions

• 1 Calorie 1000 calories
• 4.184 J 1 calorie

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Temperature

• Measured with

• Kelvin Scale The S.I. Scale
• Based on absolute zero.
• Absolute Zero The point at which the motion of
  particles of matter (their kinetic energy)
  ceases.
• K ?C 273

Fahrenheit Scale An arbitrary scale created by
Gabriel Fahrenheit. ?F (?C ? 9/5) 32
Celsius Scale Based on the freezing and boiling
points of water. ?C (?F 32) ? 5/9 ?C K
273
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Properties Changes of Matter
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Matter

• Anything that takes up space and has mass
• Can be classified as solid, liquid, gas or plasma

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Is it matter?
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What is not matter?

• ENERGY, HEAT, LIGHT, ELECTROMAGNETIC WAVES,
  MAGNETIC FIELDS, IDEAS, ETC.

Properties of Matter

• Describe the characteristics and behavior of
  matter, including the changes that matter
  undergoes

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Observing Matter

• Macroscopic Observations Observations made with
  the 5 senses

• Microscopic Observations Observations made with
  a microscope
• Submicroscopic Observations Observations of
  substances so small they cannot even be seen with
  a microscope

Macroscopic
Microscopic
Submicroscopic
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• Qualitative Observation Describes the properties
  of a substance

• Quantitative Observation An observation that
  involves a numerical value.

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Physical Properties
quantitative
characteristics
qualitative

• What are the physical properties represented in
  the image above?

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Mass

• Units grams or kilograms
• Measured with Triple Beam Balance

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VOLUME

• SI Unit cm3 or m3
• Measured with a meterstick or a metric ruler
• Common Unit mL or L
• Measured with a graduated cylinder

If the same amount of liquid is found in both of
the above containerswhich has more volume?
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States of Matter

• Depends on
• Solid
• Liquid
• Gas

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PLASMA
The most common form of matter
Free electrons and ions of an element.
Energy is needed to strip atoms of their
electrons.
Plasmas can be steered and controlled by magnetic
and electric fields.
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PLASMA TVS

• Xenon and Neon in each cell

• Intersecting electrodes charged causing electric
  current through the gas in that cell

• Electric current rapidly flowing charged
  particles causing the release of UV photons

• Photons interact with the phosphor coating giving
  off colored light

Because each cell is lit individually, the image
is bright and looks good from almost any angle.
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Chemical Properties
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Chemical Reaction A Chemical Change

• After a chemical reaction The original
  substance no longer has the same identity
• Chemical reactions can be used to

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Is it a chemical reaction?
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Law of Conservation of Matter

• Matter cannot be created nor destroyed in a
  chemical reaction.
• Developed by Antoine Lavoisier
• Mathematically
• Mass of the reactants Mass of the products
• (starting materials) (ending materials)

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PURE SUBSTANCE

• Matter with the same fixed composition and
  properties
• First Type of Pure Substance
• Element
• The Periodic Table A chart that lists the
  chemical name and chemical symbol for each
  element
• Chemical Symbol A shorthand abbreviation for
  the name of an element
• You can tell a substance is an element because it
  is on the periodic table
• -Can you separate an element? No
• Aluminum ___ Gold ____ Tin ____

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PURE SUBSTANCE

• Matter with the same fixed composition and
  properties
• Second Type of Pure Substance
• Compound
• Chemical Formula A combination of chemical
  symbols that show what elements make up a
  compound and the number of atoms of each element
• Subscript A number written to the lower right
  of an element symbol to indicate the number of
  atoms of that
• How do you know if a substance is a compound? If
  it is 1 thing onlyand it is not on the periodic
  table.
• Can you separate a compound? Yesby chemically
  decomposing it.
• NaH2CO3 Mg(OH)2

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Decomposing a Compound

• Electrolysis
• To tear apart with electricity
• The process in which electrical energy causes a
  non-spontaneous chemical reaction to occur
• May break a compound apart into its elements
• Electrolysis of PbBr2 ZnCl2
• Electrolysis of Water

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MIXTURES

• Two or more elements physically combined.
• How can you tell something is a mixture?
• It can be physically separated into its parts.

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Heterogeneous Mixtures

• The prefix hetero means different
• A mixture with different compositions throughout
• You can see each phase (part) of the mixture

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Homogeneous Mixtures

• The prefix homo- means the same
• A mixture that is the same throughout
• You cannot see the phases (parts) of the mixture.

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ALLOY
NAME OF ALLOY MAKE UP EXAMPLE
Stainless Steel 73-79 Fe 14-18 Cr 7-9 Ni
Sterling Silver 92.5 Ag 7.5 Cu
18-karat white gold 75 Au 12.5 Ag 12.5 Cu
14 karat gold 58 Au 14-28 Ag 14-28 Cu
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Solutions

• Solute The substance being dissolved in a
  solution
• Solvent The substance that dissolves the solute
• Aqueous Solution A solution in which water is
  the solvent

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HETEROGENEOUS OR HOMOGENEOUS?
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What is the solute?What is the solvent?
82 Fe 18 Cr
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Methods to Separate Mixtures

• Filtration Separates a solid from a liquid

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Separating

• Magnet Separates Fe, Co, or Ni

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Separating

• Distillation Separates two or more liquids with
  different boiling points.

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Separating

• Crystallization Separates crystalline solids
  from a saturated liquid

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Separating

• Chromatography Separates different types of
  liquids