Class notes
Thermochemistry
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- University Of Ottawa (U Of O )
Introduction to thermochemistry
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Pre LectureCalorimetery ConstantV
Ex 2C0t0z 2C0z 298K
Under constant V Underconstant P
U
qtw q Psv w Pav snRT
DU _qu w
Cnf ni RT
DU 563.5kJ mo1 2.5 KJlmol
Uv Up b
iqu qpt
563 SK mol qpt2.5kJ
mo qp
S66KJ mol
Enthalpy
AH is the change in heat for a system constant pressure
sH qp sUtPsV
Exothermic heat is given out Creleased Constantvolomeq
Endothermic heat is taken in absorbed
q nqsT
Constant Vvs Constant P
Const P nocg ConstP dn 0 ConstP Brito Const V
dU sH sU DH BUSH AU
w
qv
, Thermochemical Equations
A balanced equation that includes is Hr
the enthalpychangeColt of a reaction is written to the right of the equation
Ek HzOleg It 2cg t 4202cg sHr 1286kglmol
Types of reaction
combustion fuel
General equation i CxHy ta Oz bCO2 to H2O heat
always exothermic
If fuel has other elements presentCN s P
they will have additional
products but will always have CO2 2 Azo if combustion is complete
If S is present soo will be produced
N N02 or Nog will be produced
Solution
Ex NHyN03 csg NHyt aq t
Nos cap
12h22011 s GzH22011 Caq
the process of dissolving a puresolute in solvent often water
typically will be represented in the state labels
Can't predict if endothermic or exothermic
Neutralization
Ex NaOHcaq HCl caq NaCl caq t Hzoce
base acid salt water
Ran btwn a strong acids base
weak acidlbases result in buffered soI
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