copyright©2000 by houghton mifflin company. all rights reserved. 1 energy the capacity to do work...
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Copyright©2000 by Houghton Mifflin Company. All rights reserved. 3 The Two Types of Energy Potential: due to position or composition - can be converted to work Kinetic: due to motion of the object KE = 1 / 2 mv 2 (m = mass, v = velocity)TRANSCRIPT
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1
Energy
The capacity to do work or to produce heat.
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2
Law of Conservation of Energy
Energy can be converted from one form to another but can neither be created nor destroyed.
(Euniverse is constant)
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3
The Two Types of Energy
Potential: due to position or composition - can be converted to work
Kinetic: due to motion of the object
KE = 1/2 mv2
(m = mass, v = velocity)
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4
Temperature v. Heat
Temperature reflects random motions of particles, therefore related to kinetic energy of the system.
Heat involves a transfer of energy between 2 objects due to a temperature difference
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5
State Function
Depends only on the present state of the system - not how it arrived there.
It is independent of pathway.
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6
System and Surroundings
System: That on which we focus attention
Surroundings: Everything else in the universe
Universe = System + Surroundings
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7
Exo and Endothermic
Heat exchange accompanies chemical reactions.
Exothermic: Heat flows out of the system (to the surroundings).
Endothermic: Heat flows into the system (from the surroundings).
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8
Figure 6.2The Combustion of Methane
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9
Figure 6.3: The Energy Diagram for the Reaction of Nitrogen and Oxygen to Form Nitric Oxide
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10
First Law
First Law of Thermodynamics:
The energy of the universe is constant.
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11
First Law
E = q + w
E = change in system’s internal energyq = heatw = work
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12
Work
work = force distance
since pressure = force / area,
work = pressure volume
wsystem = PV
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13
Figure 6.4The Volume of a Cylinder
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14
EnthalpyEnthalpy = H = E + PV
E = H PVH = E + PV
At constant pressure,qP = E + PV,
where qP = H at constant pressure
H = energy flow as heat (at constant pressure)
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15
Heat Capacity
C = heat absorbedincrease in temperature
= JC
or JK
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16
Some Heat Exchange Terms
specific heat capacityheat capacity per gram = J/°C g or J/K g
molar heat capacityheat capacity per mole = J/°C mol or J/K mol
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17
Hess’s Law
Reactants Products
The change in enthalpy is the same whether the reaction takes place in one step or a series of steps.
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18
Calculations via Hess’s Law
1. If a reaction is reversed, H is also reversed.
N2(g) + O2(g) 2NO(g) H = 180 kJ
2NO(g) N2(g) + O2(g) H = 180 kJ
2. If the coefficients of a reaction are multiplied by an integer, H is multiplied by that same integer.
6NO(g) 3N2(g) + 3O2(g) H = 540 kJ
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19
Standard Enthalpies of Formation• See the C(gr) → C(d) example.
• The standard enthalpy of formation (H˚f)
of a compound is the change in enthalpy that accompanies the formation of one mole of the compound from its elements with all substances in their standard states.
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20
Standard States
Compound For a gas, pressure is exactly 1 atmosphere. For a solution, concentration is exactly 1 molar. Pure substance (liquid or solid), it is the pure liquid or
solid.
Element The form [N2(g), K(s)] in which it exists at 1 atm and
25°C.
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21
Change in Enthalpy
Can be calculated from enthalpies of formation of reactants and products.
Hrxn° = npHf(products) nrHf(reactants)
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22
Equation (6.1)H˚
rxn = ΣnpH˚f (products) - ΣnrH˚
f (reactants)
Elements are not included in this calculation because elements require no change in form.
• You can find H˚f values on p. A-21,
appendix.• See the methods box on p. 263.See S/E 6.9, p 264: let’s do this using 6.1
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23
Figure 6.11Energy Sources Used in the
United States
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24
An Opinion
• It has been proposed that the vast coal deposits formed from plants once living in the carboniferous period have resulted from the absence of any life on earth, especially the fungi or certain saprophytic bacteria, that possessed the ability to digest cellulose.
• So, they just piled up and were eventually buried… today’s coal.
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25
Figure 6.12The Earth’s Atmosphere
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26
Figure 6.13Atmospheric CO2 Concentration
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27
Figure 6.14 Coal Gasification