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Chapter 1: Thermochemistry - Coggle Diagram
Chapter 1: Thermochemistry
First Law of Thermodynamics: ∆E = Q + W
W = -PΔV
Q = m x Cs x ΔT
System & Surroundings
Exothermic
- heat: system -> surroundings
Example: condensation of water
Endothermic
- heat: surroundings -> system
Example: ice cubes melting
Enthalpy
- heat content of substance
+ΔH = endothermic
-ΔH = exothermic
Enthalpy of reaction, ΔH = −(Q /
moles of limiting reactant)
Standard enthalpy change,
ΔH°
1 atm
1.0M
298 K
Standard enthalpy of
formation
,
ΔH°f
1 mole of substance formed from its elements
Standard enthalpy of
combustion
,
ΔH°c
1 mole of compound completely burned in excess oxygen
Standard enthalpy of
neutralization
,
ΔH°n
1 mole of H+ react w/ one mole of OH- to form 1 mole of water
Standard enthalpy of
atomization
,
ΔH°a
1 mole of gaseous atoms formed from its elements
Bond
enthalpy,
ΔH°bond
to break 1 mole of bond to give gaseous atoms
Standard
lattice
enthalpy,
ΔH°latt
1 mole of crystalline solid formed from its gaseous ions
Factors: charge and ionic radius
Standard enthalpy of
solution
,
ΔH°soln
1 mole of solute is dissolved in excess water to form dilute solution
ΔH°soln = +ΔH°latt + ΔH°hyd
Enthalpy of
hydration
,
ΔH°hyd
1 mole of gaseous ions dissolve in water to form aqueous ions
Hess's Law
ΔH(rxn) = ΣΔH°f(products) - ΣΔH°f(reactants)
Born-Haber Cycle
ΔH°f = ΔHa + ΔH(ion) + ΔH(affinity) + ΔH(lattice)