Chapter 9 Chemical Reactions I.Classification of Chemical Reactions
Please Pick Up Chemical Reactions Problem Set..
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Please Pick Up
Chemical Reactions Problem Set.
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ThermochemistryFirst Law of Thermodynamics
Edward A. Mottel
Department of Chemistry
Rose-Hulman Institute of Technology
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04/19/23
Chemical Thermodynamics
Reading assignment: • Chang: Chapter 6.1-6.3
A study of the energy changes which accompany the physical and chemical changes of matter.
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A Thermodynamic Term
Enthalpy
The total heat energy contentof a molecule.
If a chemical processrequires heat,the enthalpy changeis endothermic.
If a chemical processreleases heat,
the reaction changeis exothermic.
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Solution ReactionsEndothermic and Exothermic
NH4+(aq) + NO3
–(aq)
Hsoln = +25.8 kJmol–1
2 H+(aq) + SO42–(aq)
Hsoln = -96.2 kJmol–1
exothermic
NH4NO3(s)H2O
H2SO4(conc)H2O
enthalpy of solution endothermic
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Changes in Physical StateReactions should be balanced and
annotated
Enthalpy of vaporization of water
Enthalpy of sublimation of water
Enthalpy of fusion of water
H2O(g) H2O(l)
H2O(g) H2O(s)
H2O(l) H2O(s)
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Chemical ReactionsExamples
Decomposition
Single replacement
Double replacement
Cr2O3(s) + N2(g) + 4 H2O(g) (NH4)2Cr2O7(s)
2 NaCl(aq) + I2(aq)2 NaI(aq) + Cl2(g)
NaCl(aq) + H2CO3(aq) HCl(aq) + NaHCO3(s)
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Chemical ReactionsCombustion and Formation
Combustion
Formation
2 CO2(g) + 3 H2O(g) C2H5OH(l)+ 3 O2(g)
Na2CO3(s)2 Na(s) + C(gr) + 3/2 O2(g)
carbon is converted to
hydrogen is converted to
most common elemental form
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Combustion of sucrose (C12H22O11)
Formation of sucrose
12 CO2(g) + 11 H2O(g) C12H22O11(s) + 12 O2(g)
C12H22O11(s)12 C(gr) + 11 H2(g) + 11/2 O2(g)
Write the equationfor each of the following processes
more examples
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Thermodynamic Terms
Heat, q. Work, w. Internal energy, E or U System Surroundings Enthalpy, H State Functions
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Thermal Energy
q
What is the difference betweenheat and temperature?
Are heat and temperatureintensive or extensive properties?
Heat flows form a warmer body to a cooler body.
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Work
FFFFFFFFFFFFFFFFFFFFFFFFw = F·d
d
Work has an intensive and a capacitive factor.
What is the difference betweenwork and being tired?
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Work
Type of Work
mechanical
expansion
electrical
Intensity
force
pressure
potentialdifference
Capacity
distance
volume change (dV)
amount of electricity(charge)
gravitational gravity height x mass
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Internal Energy
E or U The total kinetic and potential energy of a
molecule or ion• Molecular motion• Electronic changes
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Molecules Store Energy inMolecular Motion
translation
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Electronic Changes
endothermicchange in electron
energy levelsO h Otriplet oxygen singlet oxygen
OH H OH H
exothermicbond formation
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First Law of Thermodynamics
U = energygained - energylost
The change in internal energy of a system isequal to the energy added to the system,
minus the energy lost by the system.
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25 ºC200 ºC400 ºC800 ºC
E = q + w
First Law of Thermodynamics
The change in internal energyis equal to the heat added and the work done on the system.
What’s happeningto the gas
in the rigid bulb?
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Closed system Isolated system
q
Surroundings - Everything else(the rest of the universe).
System - any region of space or materialwhich is considered in dealing with
energy changes that matter undergoes.
mm
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Internal Energy
translation
The total energy (E or U) of a molecule or ionis due to all sources of kinetic and potential energy.
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1.0 atm1.1 atm 1.2 atm 1.3 atm 1.4 atm 1.5 atm 1.6 atm 1.7 atm 1.8 atm 2.0 atm 2.3 atm 2.7 atm 3.2 atm
First Law of Thermodynamics
E = q + w
4.0 atm
What’s happening to the temperature of the gas?Why?
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First Law of Thermodynamics
E = q + w
Explain what is happeningusing the First Law of Thermodynamics.
1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm1.0 atm
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