The temperature dependences of the
heat capacity of two crystalline
polycyclic aromatic hydrocarbons, benz[a]anthracene and chrysene,
were investigated using adiabatic calorimetry in the temperature ranges T = 5.5–326.4 and 5.7–328.1 K, respectively.
Smoothed heat capacity, C
p, m
o(T), values between 0 and 320 K are presented, along with values for
the standard thermodynamic functions: the enthalpy, H
m
o(T) – H
m
o(0), the entropy, S
m
o(T), and the Gibbs free energy, G
m
o(T) – H
m
o(0). Using the heat capacity, C
p, m
o(T), data, the standard molar third-law entropies at T = 298.15 K, S
m
o, are calculated to be 272.1 ± 1.6
J·K–1·mol–1 for benz[a]anthracene
and 274.1 ± 1.7 J·K–1·mol–1 for chrysene. The standard enthalpies of combustion, Δc
H
m
o, for benz[a]anthracene and chrysene have been
determined using an isothermal combustion calorimeter with a stationary
bomb. These new experimental results, together with literature data,
are used to calculate the enthalpies of formation, Δf
H
m
o, and Gibbs free energies of formation, Δf
G
m
o, giving Δf
H
m
o(298.15 K, benz[a]anthracene,
cr) = 143.3 ± 22.3 kJ · mol–1 and Δf
G
m
o(298.15 K, benz[a]anthracene, cr) = 326.8 ±
22.4 kJ · mol–1 for benz[a]anthracene and Δf
H
m
o(298.15 K, chrysene, cr) = 110.7 ± 13.0
kJ · mol–1 and Δf
G
m
o(298.15 K,
chrysene, cr) = 293.6 ± 13.2 kJ · mol–1 for chrysene.