What happens to thermal (heat) energy? - PowerPoint PPT Presentation

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What happens to thermal (heat) energy?

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Thermodynamics Calculating Heat Production Heat of Formation Heat of Formation: The general idea Find the enthalpy change for burning ethyl alcohol ... – PowerPoint PPT presentation

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Title: What happens to thermal (heat) energy?


1
Thermodynamics
2
Energy is neither created or destroyed during
chemical or physical changes, but it is
transformed from one form to another.?Euniverse
0
3
TYPES of ENERGY Kinetic Potential Mechanical
Gravitational Thermal Electrostatic Electrical
Chemical Radiant
Energy Conversion Examples 1. dropping a
rock 2. using a flashlight 3. driving a car
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SYSTEMS and SURROUNDINGS System The thing
under study Surroundings Everything else in the
universe Energy transfer between system and
surroundings
Endo heat added to system Exo heat released by
system
6
HEAT What happens to thermal (heat) energy?
  • Three possibilities
  • Warms another object
  • Causes a change of state
  • Is used in an endothermic reaction

7
Temperature Changes from Heat Exchange
Example 1 5 g wood at 0 oC 5 g wood at
100 oC Example 2 10 g wood at 0 oC 5 g
wood at 100 oC Example 3 5 g copper at 0 oC
5 g copper at 100 oC Example 4 5 g wood at 0
oC 5 g copper at 100 oC
Choices 1 0 oC 2 33 oC 3 50 oC 4.
67 oC 5 100 oC 6 other
8
What happens to thermal (heat) energy?
  • When objects of different temperature meet
  • Warmer object cools
  • Cooler object warms
  • Thermal energy is transferred
  • qwarmer -qcooler

9
Quantitative Calculating Heat Exchange Specific
Heat Capacity
10
Specific Heat Capacity
  • The energy required to heat one gram of a
    substance by 1 oC.
  • Usefulness J transferred S.H. x g x ?T
  • How much energy is used to heat 250 g water from
    17 oC to 100 oC?

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What happens to thermal (heat) energy?
  • When objects of different temperature meet
  • Warmer object cools
  • Cooler object warms
  • Thermal energy is transferred
  • qwarmer -qcooler
  • specific heat x mass x ?T specific heat x mass
    x ?T
  • warmer object
    cooler object

13
Heat transfer between substances
14
Conceptually Easy Example with Annoying
Algebra If we mix 250 g H2O at 95 oC with 50 g
H2O at 5 oC, what will the final temperature be?
15
Thermal Energy and Phase Changes
First What happens?
16
Thermal Energy and Phase Changes
First What happens?
17
Thermal Energy and Phase Changes
First What happens?
18
But whats really happening?
  • Warming
  • Molecules move more rapidly
  • Kinetic Energy increases
  • Temperature increases
  • Melting/Boiling
  • Molecules do NOT move more rapidly
  • Temperature remains constant
  • Intermolecular bonds are broken
  • Chemical potential energy (enthalpy) increases

19
Energy and Phase Changes
Quantitative Treatment
Melting Heat of Fusion (DHfus) for Water 333
J/g Boiling Heat of Vaporization (DHvap) for
Water 2256 J/g
20
Total Quantitative Analysis
Convert 40.0 g of ice at 30 oC to steam at 125 oC
Warm ice (Specific heat 2.06 J/g-oC)
Melt ice
Warm water (s.h. 4.18 J/g-oC)
21
Total Quantitative Analysis
Convert 40.0 g of ice at 30 oC to steam at 125 oC
Boil water
Warm steam (s.h. 1.92 J/g-oC)
22
Energy and Chemical Reactions
Lots of different types of energy.We use
EnthalpyHeat exchanged under constant pressure.
23
Energy/Enthalpy Diagrams
24
Some Examples of Enthalpy Change
2 C(s) 2 H2(g) ? C2H4(g) ?H 52 kJ
25
Enthalpy Change and Chemical Reactions
DH is usually more complicated, due to solvent
and solid interactions. So, we measure DH
experimentally. Calorimetry Run reaction in a
way that the heat exchanged can be measured. Use
a calorimeter.
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27
Bomb Calorimetry Experiment
N2H4 3 O2 ? 2 NO2 2 H2O Energy released E
absorbed by water E absorbed by
calorimeter Ewater Ecalorimeter Total E
?H energy/moles
0.500 g N2H4 600 g water 420 J/oC
28
Enthalpy Change and Bond Energies
DH energy needed to break bonds energy
released forming bondsExample formation of
water
DH 498 (2 x 436) 4 x 436 kJ -482 kJ
29
General Rule
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SO2 ½ O2 ? SO3 dH -98.9 kJ2 SO3 ? 2 SO2
O2 dH ?
32
Hesss Law
If reactions can be added so can their ?H
values.
33
Thermochemistry Lab Calculations Goal What is
?H for the formation of MgO from Mg(s) and
O2(g)? Mg(s) ½ O2(g) ? MgO(s) ?H ?
kJ/mol Data From lab measurements Mg(s) 2
H(aq) ? Mg2(aq) H2(g) ?H1 ___________
kJ/mol MgO(s) 2 H(aq) ? Mg2(aq) H2O(l)
?H2 ___________ kJ/mol From a table
H2(g) ½ O2(g) ? H2O(l) ?H3 -285.8
kJ/mol Task Find a way to add these three
reactions to get the desired reaction. Manipulate
the ?H values as needed, and add them.
34
Calculating Heat Production
35
Heat of Formation
36
Heat of Formation The general idea
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38
Find the enthalpy change for burning ethyl alcohol
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