chapter 9 energy and hydrocarbons. chapter outline background & energy from fuels alkanes:...
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Chapter 9
Energy and Hydrocarbons
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Chapter Outline
Background & Energy from FuelsAlkanes: Backbone of Organic ChemistryAlkenes and Alkynes: Reactive cousins of AlkanesCyclic HydrocarbonsPetroleumNatural GasCoalMethanol (Gasohol)
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Define some terms
Energy is a common idea that ran through the first half of the class. – What is Energy?– What is Heat?– What is Temperature?– What is the difference between heat and temperature? – What are the ‘units’ of each measurement?– Exothermic vs. Endothermic
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Energy
Energy is defined as ‘the capacity to do work’– What does this mean to you?
Energy: Capacity to do work or to transfer heat!
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Types of Energy
Kinetic Energy – Energy of Motion
Ek = ½ mv2 m= mass (kg)
v = velocity (m/s)Ek = Joules
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Potential Energy – Stored energy based on the position of one object with respect to another
Ep = m *g* h m = mass (kg)g = gravitational constant = 9.806 m/s2
h= distance above reference
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Example
What is the kinetic Energy of a bowling ball moving at a velocity of 1.5 m/s? (Mass of bowling ball = 7.5 kg)
Ek = ½ mv2
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Units of Energy
Heat can have the following units– Joules (J) = 1 kg*m2/s2
– Kilojoules(kJ)– calories (cal) = 4.184 Joule– Kilocalories (kcal) = 1000 calories– Dietary Calories = Calories (Cal) = 1 kcal– Erg– BTU– Foot-pounds
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Energy
Calculate the amount of potential energy of a 1 kg book raised about 6 ft (~2 meters) into the air.
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First Law of Thermodynamics
Energy is neither created nor destroyed. – The Energy is said to be “transferred or
transformed”!
What happened to the energy of the book?
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Heat vs. Temperature
Some of the energy was transformed to sound energy and some converted to heat!
WHAT IS HEAT?– Before we consider heat … let’s look at temperature!
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Temperature
Think back to global warming – vibrating molecules caused an increase in
temperature
Temperature – average kinetic energy of molecules in a substance.
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What is Heat?
Heat is the total amount of energy in a substance– In other words – its the amount of thermal energy that a
system contains.
Heat Energy = (specific heat)*(amount of substance)*(Temperature)
What’s the difference between Heat and Temperature?Think of this Example – A drop of boiling water and 4 liters of boiling water. Which one has more energy?
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What is a calorie?
Based on the work of James Joule (late 1800’s)– One calorie = amount of heat required to raise 1
gram of water 1 degree Celsius.
– One calorie = 4.184 Joules
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Units of Energy
Heat can have the following units– Joules (J) = 1 kg*m2/s2
– Kilojoules(kJ)– calories (cal) = 4.184 Joule– Kilocalories (kcal) = 1000 calories– Dietary Calories = Calories (Cal) = 1 kcal– Erg– BTU– Foot-pounds
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Some ‘exercises’
1. How many joules are in 425 Cal?2. How much energy is required to raise 1 gram of
water 1oC?3. How much energy is required to raise 1000
grams (1 kg) of water from room temperature (25oC) to boiling (100oC) ?
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Exothermic vs. Endothermic
Draw energy diagrams for the following processes.– Dissolving of Urea in water– Dissolving of Ethanol in water
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9.1 Energy from Fuels
Petroleum38%
Nuclear8%
Coal23%
Natural Gas24%
Renewable7%
Most of our energy comes from Fossil Fuels (Petroleum, Coal, Natural Gas)
Source of Energy used in the United States - 2000
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Combustion of Natural Gas
Natural Gas is mostly Methane
Consider the complete combustion of methane ____ CH4 + ____ O2 -> ____ CO2 + ____ H2O
Methane Oxygen Carbon dioxide Water
Is Energy Produced? How much?
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What determines if Energy is released or absorbed in a chemical reaction?
Bond Energies!!
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BOND ENERGIESSingle BondsH C N O S F Cl Br I
H 432C 411 346N 386 305 167O 459 358 201 142S 363 272 - - 226F 565 485 283 190 284 155Cl 428 327 313 218 255 249 240Br 362 285 - 201 217 249 216 190I 295 213 - 201 - 278 208 175 149
Multiple BondsC=C 602 C=N 615 C=O 1072C=C 835 N=O 607N=N 418 O=O 494N=N 942 C=O 799
Bond Energies are given in kJ/mole
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