thermochemistry cp unit 9 chapter 17 thermochemistry 17.1 thermochemistry is the study of energy...
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THERMOCHEMISTRY
CP Unit 9Chapter 17
Thermochemistry 17.1 Thermochemistry is the study of energy
changes (HEAT) that occur during chemical reactions and changes in state.
ENTHALPY 17.2 Enthalpy = a type of chemical energy, sometimes
referred to as “heat content”, ΔH (the heat of reaction for a chemical reaction)
endothermic reactions (feels cold): q = ΔH > 0 (positive values)
exothermic reactions (feels hot): q (heat) = ΔH (enthaply, heat of rxn) < 0 (negative
values)
Endo vs. Exo-Endothermic reactions:
absorbs heat from surroundings (+). If you touch an
endothermic reaction it feels COLD
Exothermic reactions: release heat to the surroundings (-) If you touch an
exothermic reaction it feels HOT
Magnitude of Heat Flow Units of heat energy:
1 kcal = 1,000 cal = 1 Cal (nutritional) 1 kJ = 1,000 J 1 calorie = 4.184 J 1 kcal = 4.184 kJ
Thermochemical Equations A chemical equation that shows the
enthalpy (H) is a thermochemical equation.
Rule #1The magnitude (value) of H is directly proportional to the amount of reactant or product.
H2 + Cl2 2HCl H = - 185 kJ
* meaning there are 185 kJ of energy RELEASED for every:1 mol H2
1 mol Cl22 moles HCl
Rules of ThermochemistryExample 1: H2 + Cl2 2HCl H = - 185 kJ
Calculate H when 2.00 moles of Cl2 reacts.
Rules of ThermochemistryExample 2: Methanol burns to produce carbon dioxide and water:
2CH3OH + 3O2 2CO2 + 4H2O H = - 1454 kJ
What mass of methanol is needed to produce 1820 kJ?
Rule #2 H for a reaction is equal in the magnitude but opposite in sign to H for the reverse reaction.
(If 6.00 kJ of heat absorbed when a mole of ice melts, then 6.00 kJ of heat is given off when 1.00 mol of liquid water freezes)
Rules of ThermochemistryExample 1: Given: H2 + ½O2 H2O H = -285.8 kJ
Reverse: H2O H2 + ½O2 H = +285.8 kJ
Example 2CaCO3 (s) CaO (s) + CO2 (g) H = 178 kJ
What is the H for the REVERSE RXN?
CaO (s) + CO2 (g) CaCO3 (s) H = ?
Alternate form of thermochem. eq. Putting the heat content of a reaction INTO
the actual thermochemical eq. H2 + ½O2 H2O H = -285.8 kJ
Exothermic
(H is negative)
Heat is RELEASED as a PRODUCT
The alternate form is this:
H2 + ½O2 H2O +285.8 kJ
EX:2 NaHCO3 + 129 kJ Na2CO3 + H2O + CO2
Put in the alternate form
The alternate form is this:
2 NaHCO3 Na2CO3 + H2O + CO2 H = + 129 kJ
Put the following in alternate form1. H2 + Cl2 2 HCl H = -185 kJ
2. 2 Mg + O2 2 MgO + 72.3 kJ
3. 2 HgO 2 Hg + O2 H = 181.66 kJ
Enthalpies of Formation
enthalpy
change (delta)
standard condition
s
formation
fH
Enthalpies of Formation usually exothermic see table for Hf
value (Table A3) enthalpy of formation of an element
in its stable state = 0 these can be used to calculate H
for a reaction
Standard Enthalpy Change
Standard enthalpy change, H, for a given thermochemical equation is = to the sum of the standard enthalpies of formation of the product – the standard enthalpies of formation of the reactants.
) H(-) H(H reactantsfproductsfrxn
sum of (sigma)
Standard Enthalpy Change elements in their standard states can be omitted:
2 Al(s) + Fe2O3(s) 2 Fe(s) + Al2O3(s)
ΔHrxn = (ΔHfproducts) - (ΔHf
reactants)
ΔHrxn = ΔHfAl2O3 - ΔHf
Fe2O3
ΔHrxn = (-1676.0 kJ) – (-822.1 kJ)
ΔHrxn = -853.9 kJ
Standard Enthalpy Change the coefficient of the products and reactants in
the thermochemical equation must be taken into account:
O2(g) + 2SO2 (g) 2SO3 (g)
ΔHrxn = (ΔHfproducts) - (ΔHf
reactants)
ΔHrxn = 2ΔHfSO3 - 2ΔHf
SO2
ΔHrxn = 2(-395.7 kJ) – 2(-296.8 kJ)
ΔHrxn = -197.8 kJ
Standard Enthalpy Change - Calculate the standard heat for formation of benzene, C6H6, given the following thermochemical equation:
C6H6(l) + 15/2 O2(g) 6CO2(g) + 3H2O(l) H = -3267.4 kJ
-3267.4kJ = [6(-393.5kJ)+3(-285.8kJ)]–X
X = +49.0 kJ
-3267.4kJ = -3218.4–X
-49.0kJ = – X
X Total-393.5kJ -285.8kJ
Don’t forget the coefficents!